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Sofia
2/24/2023
AP Chemistry
Autopyrolysis of Water
14
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Feb 24, 2023
•
The pH scaleis a fundamental concept in chemistry that... Show more
Water exhibits a fascinating property called Autoprotolysis, where it acts as both an acid and base. This dual nature makes water an ampholyte - a substance that can donate or accept protons. The self-ionization of water produces hydronium (H3O+) and hydroxide (OH-) ions in a delicate equilibrium.
Definition: Water autoprotolysis is the chemical reaction where two water molecules react to form hydronium and hydroxide ions: H2O + H2O ⇌ H3O+ + OH-
The ion product constant of water (Kw) at 25°C is 1 x 10-14, representing the product of hydronium and hydroxide ion concentrations. In pure water, [H3O+] equals [OH-] at 1 x 10-7 M, creating a neutral solution. This fundamental concept leads us to the pH scale, developed by Søren Sørensen in 1909.
What does pH stand for? The term pH represents "potential of hydrogen" and measures the concentration of hydrogen ions in a solution. The pH scale ranges from 0 to 14, where pH < 7 indicates acidic solutions, pH = 7 represents neutral solutions, and pH > 7 indicates basic solutions. The mathematical relationship between pH and concentration is logarithmic: pH = -log[H3O+].
Highlight: The relationship between pH and concentration follows an inverse logarithmic pattern - for every unit decrease in pH, the hydrogen ion concentration increases tenfold.
Understanding the strength of acids and bases requires examining their dissociation constants (Ka and Kb). Starke und schwache Basen (strong and weak bases) and their acidic counterparts behave differently in solution based on their dissociation extent.
Example: Strong acids like HCl dissociate completely in water: HCl + H2O → H3O+ + Cl- (100% ionization) Weak acids like CH3COOH partially dissociate: CH3COOH + H2O ⇌ H3O+ + CH3COO- (partial ionization)
Schwache Säuren Beispiele (examples of weak acids) include acetic acid (Ka = 1.8 x 10-5) and nitrous acid (Ka = 4.5 x 10-4). These acids establish equilibrium in solution, with only a fraction of molecules ionizing. The strength of acids and bases can be categorized based on their Ka and Kb values:
The common ion effect demonstrates how adding an ion common to an equilibrium system affects the dissociation of a weak electrolyte. This principle has important applications in buffer solutions and pH control.
When sodium acetate (NaCH3COO) is added to an acetic acid solution, the additional acetate ions (CH3COO-) shift the equilibrium toward the undissociated acid, reducing the hydrogen ion concentration and increasing pH. This follows Le Chatelier's Principle.
Vocabulary: The common ion effect refers to the suppression of ionization of a weak electrolyte by adding a strong electrolyte that contains an ion in common with the weak electrolyte.
The mathematical treatment involves considering both the initial concentrations and the equilibrium shifts. For example, adding sodium acetate to a 0.2 M acetic acid solution reduces the hydrogen ion concentration and increases the pH, demonstrating the practical application of the common ion effect in buffer solutions.
Understanding pH calculations is crucial for various applications in chemistry and biology. The relationship between pH, pOH, and pKw follows the equation: pH + pOH = 14 (at 25°C).
For strong acids and bases, pH calculations are straightforward since they dissociate completely. However, weak acids and bases require considering the equilibrium constant and applying the ICE table method (Initial, Change, Equilibrium).
Example: For a 0.1 M weak acid with Ka = 1.8 x 10-5: Initial: [HA] = 0.1 M Let x = [H+] produced Equilibrium: Ka = [H+][A-]/[HA] = (x)(x)/(0.1-x)
The Säure-Basen-Haushalt (acid-base balance) in biological systems relies heavily on these principles, particularly in maintaining blood pH and proper cellular function. Understanding these calculations helps in various fields, from environmental science to medical diagnostics.
A buffer solution is a specialized mixture that maintains a stable pH when small amounts of acids or bases are added. This remarkable property makes buffers essential in biological systems and industrial processes where pH control is critical.
Definition: A buffer solution consists of a weak acid and its salt, or a weak base and its salt, working together through the common-ion effect to resist pH changes.
The buffer capacity represents how much acid or base a buffer can neutralize before significant pH changes occur. There are two main types of buffers:
Highlight: Buffer solutions are crucial in:
The human body relies on several buffer systems to maintain precise pH levels. The pH scale, discovered by Søren Sørensen in 1909, helps measure these delicate acid-base balances.
Example: Blood pH must stay remarkably close to 7.4. Even small deviations can be dangerous:
Key biological buffer systems include:
Vocabulary: Ampholytes are molecules that can act as both acids and bases, making them excellent biological buffers.
The Henderson-Hasselbalch equation provides a mathematical framework for calculating buffer pH:
pH = pKa + log([base]/[acid])
This equation shows the relationship between:
Definition: The equation helps predict how buffer composition affects pH and can be used to design buffers with specific pH values.
For acid buffers: pH = pKa + log([salt]/[weak acid]) For base buffers: pOH = pKa + log([salt]/[base])
Buffer solutions find extensive use across multiple fields:
Example: A common buffer preparation involves mixing 1.0M acetic acid with 1.0M sodium acetate to create a buffer with pH 4.76, which remains stable even when small amounts of acid or base are added.
The Brønsted-Lowry concept fundamentally transformed our understanding of acid-base chemistry by focusing on proton transfer reactions. In this framework, acids and bases are defined by their behavior during chemical reactions rather than just their properties in isolation. An acid serves as a proton donor, while a base acts as a proton acceptor, creating a dynamic relationship that underlies countless chemical processes.
Definition: A conjugate acid-base pair consists of two chemical species that differ by exactly one proton (H+). When an acid donates its proton, it becomes its conjugate base. Similarly, when a base accepts a proton, it becomes its conjugate acid.
The relationship between acids and bases extends beyond simple proton transfer. Ampholytes are species that can act as either acids or bases depending on the reaction conditions, demonstrating the contextual nature of acid-base behavior. This concept is crucial for understanding biological systems, where many molecules must maintain precise pH balance through amphoteric behavior.
The solubility product principle represents a specialized application of chemical equilibrium laws to heterogeneous systems. This principle specifically addresses situations involving slightly soluble electrolytes and their saturated solutions. When a solid ionic compound dissolves in water, it establishes an equilibrium between the solid phase and its ions in solution. The mathematical expression of this equilibrium, known as the solubility product constant (Ksp), provides a quantitative measure of solubility.
Example: Consider silver chloride (AgCl) dissolving in water: AgCl(s) ⇌ Ag+(aq) + Cl-(aq) The solubility product expression would be: Ksp = [Ag+][Cl-]
The concept of pH, developed by Soren Sorensen in 1909, revolutionized our understanding of acid-base chemistry. The pH scale provides a logarithmic measure of hydrogen ion concentration in aqueous solutions, ranging from 0 to 14. This scale is fundamental to chemistry, biology, and numerous industrial applications.
Vocabulary: The Ionenprodukt des Wassers (ion product of water) represents the equilibrium constant for water's self-ionization, written as Kw = [H+][OH-] = 1.0 × 10^-14 at 25°C.
Understanding the relationship between pH and concentration is crucial for various applications. The logarithmic nature of the pH scale means that each unit change represents a tenfold difference in hydrogen ion concentration. This mathematical relationship helps explain why small changes in pH can have significant effects in biological systems and chemical processes.
The concept of Autoprotolyse (autoprotolysis) explains how water molecules can act as both acid and base, transferring protons between themselves to maintain equilibrium. This self-ionization of water establishes the foundation for understanding acid-base behavior in aqueous solutions and helps explain why pure water has a pH of 7 at room temperature.
Highlight: The pH scale's logarithmic nature means that a solution with pH 4 is ten times more acidic than a solution with pH 5, and one hundred times more acidic than a solution with pH 6.
Our AI companion is specifically built for the needs of students. Based on the millions of content pieces we have on the platform we can provide truly meaningful and relevant answers to students. But its not only about answers, the companion is even more about guiding students through their daily learning challenges, with personalised study plans, quizzes or content pieces in the chat and 100% personalisation based on the students skills and developments.
You can download the app in the Google Play Store and in the Apple App Store.
That's right! Enjoy free access to study content, connect with fellow students, and get instant help – all at your fingertips.
App Store
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The app is very easy to use and well designed. I have found everything I was looking for so far and have been able to learn a lot from the presentations! I will definitely use the app for a class assignment! And of course it also helps a lot as an inspiration.
Stefan S
iOS user
This app is really great. There are so many study notes and help [...]. My problem subject is French, for example, and the app has so many options for help. Thanks to this app, I have improved my French. I would recommend it to anyone.
Samantha Klich
Android user
Wow, I am really amazed. I just tried the app because I've seen it advertised many times and was absolutely stunned. This app is THE HELP you want for school and above all, it offers so many things, such as workouts and fact sheets, which have been VERY helpful to me personally.
Anna
iOS user
I think it’s very much worth it and you’ll end up using it a lot once you get the hang of it and even after looking at others notes you can still ask your Artificial intelligence buddy the question and ask to simplify it if you still don’t get it!!! In the end I think it’s worth it 😊👍 ⚠️Also DID I MENTION ITS FREEE YOU DON’T HAVE TO PAY FOR ANYTHING AND STILL GET YOUR GRADES IN PERFECTLY❗️❗️⚠️
Thomas R
iOS user
Knowunity is the BEST app I’ve used in a minute. This is not an ai review or anything this is genuinely coming from a 7th grade student (I know 2011 im young) but dude this app is a 10/10 i have maintained a 3.8 gpa and have plenty of time for gaming. I love it and my mom is just happy I got good grades
Brad T
Android user
Not only did it help me find the answer but it also showed me alternative ways to solve it. I was horrible in math and science but now I have an a in both subjects. Thanks for the help🤍🤍
David K
iOS user
The app's just great! All I have to do is enter the topic in the search bar and I get the response real fast. I don't have to watch 10 YouTube videos to understand something, so I'm saving my time. Highly recommended!
Sudenaz Ocak
Android user
In school I was really bad at maths but thanks to the app, I am doing better now. I am so grateful that you made the app.
Greenlight Bonnie
Android user
I found this app a couple years ago and it has only gotten better since then. I really love it because it can help with written questions and photo questions. Also, it can find study guides that other people have made as well as flashcard sets and practice tests. The free version is also amazing for students who might not be able to afford it. Would 100% recommend
Aubrey
iOS user
Best app if you're in Highschool or Junior high. I have been using this app for 2 school years and it's the best, it's good if you don't have anyone to help you with school work.😋🩷🎀
Marco B
iOS user
THE QUIZES AND FLASHCARDS ARE SO USEFUL AND I LOVE THE SCHOOLGPT. IT ALSO IS LITREALLY LIKE CHATGPT BUT SMARTER!! HELPED ME WITH MY MASCARA PROBLEMS TOO!! AS WELL AS MY REAL SUBJECTS ! DUHHH 😍😁😲🤑💗✨🎀😮
Elisha
iOS user
This app is phenomenal down to the correct info and the various topics you can study! I greatly recommend it for people who struggle with procrastination and those who need homework help. It has been perfectly accurate for world 1 history as far as I’ve seen! Geometry too!
Paul T
iOS user
The app is very easy to use and well designed. I have found everything I was looking for so far and have been able to learn a lot from the presentations! I will definitely use the app for a class assignment! And of course it also helps a lot as an inspiration.
Stefan S
iOS user
This app is really great. There are so many study notes and help [...]. My problem subject is French, for example, and the app has so many options for help. Thanks to this app, I have improved my French. I would recommend it to anyone.
Samantha Klich
Android user
Wow, I am really amazed. I just tried the app because I've seen it advertised many times and was absolutely stunned. This app is THE HELP you want for school and above all, it offers so many things, such as workouts and fact sheets, which have been VERY helpful to me personally.
Anna
iOS user
I think it’s very much worth it and you’ll end up using it a lot once you get the hang of it and even after looking at others notes you can still ask your Artificial intelligence buddy the question and ask to simplify it if you still don’t get it!!! In the end I think it’s worth it 😊👍 ⚠️Also DID I MENTION ITS FREEE YOU DON’T HAVE TO PAY FOR ANYTHING AND STILL GET YOUR GRADES IN PERFECTLY❗️❗️⚠️
Thomas R
iOS user
Knowunity is the BEST app I’ve used in a minute. This is not an ai review or anything this is genuinely coming from a 7th grade student (I know 2011 im young) but dude this app is a 10/10 i have maintained a 3.8 gpa and have plenty of time for gaming. I love it and my mom is just happy I got good grades
Brad T
Android user
Not only did it help me find the answer but it also showed me alternative ways to solve it. I was horrible in math and science but now I have an a in both subjects. Thanks for the help🤍🤍
David K
iOS user
The app's just great! All I have to do is enter the topic in the search bar and I get the response real fast. I don't have to watch 10 YouTube videos to understand something, so I'm saving my time. Highly recommended!
Sudenaz Ocak
Android user
In school I was really bad at maths but thanks to the app, I am doing better now. I am so grateful that you made the app.
Greenlight Bonnie
Android user
I found this app a couple years ago and it has only gotten better since then. I really love it because it can help with written questions and photo questions. Also, it can find study guides that other people have made as well as flashcard sets and practice tests. The free version is also amazing for students who might not be able to afford it. Would 100% recommend
Aubrey
iOS user
Best app if you're in Highschool or Junior high. I have been using this app for 2 school years and it's the best, it's good if you don't have anyone to help you with school work.😋🩷🎀
Marco B
iOS user
THE QUIZES AND FLASHCARDS ARE SO USEFUL AND I LOVE THE SCHOOLGPT. IT ALSO IS LITREALLY LIKE CHATGPT BUT SMARTER!! HELPED ME WITH MY MASCARA PROBLEMS TOO!! AS WELL AS MY REAL SUBJECTS ! DUHHH 😍😁😲🤑💗✨🎀😮
Elisha
iOS user
This app is phenomenal down to the correct info and the various topics you can study! I greatly recommend it for people who struggle with procrastination and those who need homework help. It has been perfectly accurate for world 1 history as far as I’ve seen! Geometry too!
Paul T
iOS user
The pH scale is a fundamental concept in chemistry that measures the acidity or alkalinity of a solution, developed by Danish chemist Søren Sørensen in 1909 while working at the Carlsberg Laboratory.
The scale is based on the Ionenprodukt des... Show more
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Water exhibits a fascinating property called Autoprotolysis, where it acts as both an acid and base. This dual nature makes water an ampholyte - a substance that can donate or accept protons. The self-ionization of water produces hydronium (H3O+) and hydroxide (OH-) ions in a delicate equilibrium.
Definition: Water autoprotolysis is the chemical reaction where two water molecules react to form hydronium and hydroxide ions: H2O + H2O ⇌ H3O+ + OH-
The ion product constant of water (Kw) at 25°C is 1 x 10-14, representing the product of hydronium and hydroxide ion concentrations. In pure water, [H3O+] equals [OH-] at 1 x 10-7 M, creating a neutral solution. This fundamental concept leads us to the pH scale, developed by Søren Sørensen in 1909.
What does pH stand for? The term pH represents "potential of hydrogen" and measures the concentration of hydrogen ions in a solution. The pH scale ranges from 0 to 14, where pH < 7 indicates acidic solutions, pH = 7 represents neutral solutions, and pH > 7 indicates basic solutions. The mathematical relationship between pH and concentration is logarithmic: pH = -log[H3O+].
Highlight: The relationship between pH and concentration follows an inverse logarithmic pattern - for every unit decrease in pH, the hydrogen ion concentration increases tenfold.
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Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
Understanding the strength of acids and bases requires examining their dissociation constants (Ka and Kb). Starke und schwache Basen (strong and weak bases) and their acidic counterparts behave differently in solution based on their dissociation extent.
Example: Strong acids like HCl dissociate completely in water: HCl + H2O → H3O+ + Cl- (100% ionization) Weak acids like CH3COOH partially dissociate: CH3COOH + H2O ⇌ H3O+ + CH3COO- (partial ionization)
Schwache Säuren Beispiele (examples of weak acids) include acetic acid (Ka = 1.8 x 10-5) and nitrous acid (Ka = 4.5 x 10-4). These acids establish equilibrium in solution, with only a fraction of molecules ionizing. The strength of acids and bases can be categorized based on their Ka and Kb values:
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Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
The common ion effect demonstrates how adding an ion common to an equilibrium system affects the dissociation of a weak electrolyte. This principle has important applications in buffer solutions and pH control.
When sodium acetate (NaCH3COO) is added to an acetic acid solution, the additional acetate ions (CH3COO-) shift the equilibrium toward the undissociated acid, reducing the hydrogen ion concentration and increasing pH. This follows Le Chatelier's Principle.
Vocabulary: The common ion effect refers to the suppression of ionization of a weak electrolyte by adding a strong electrolyte that contains an ion in common with the weak electrolyte.
The mathematical treatment involves considering both the initial concentrations and the equilibrium shifts. For example, adding sodium acetate to a 0.2 M acetic acid solution reduces the hydrogen ion concentration and increases the pH, demonstrating the practical application of the common ion effect in buffer solutions.
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Join milions of students
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Understanding pH calculations is crucial for various applications in chemistry and biology. The relationship between pH, pOH, and pKw follows the equation: pH + pOH = 14 (at 25°C).
For strong acids and bases, pH calculations are straightforward since they dissociate completely. However, weak acids and bases require considering the equilibrium constant and applying the ICE table method (Initial, Change, Equilibrium).
Example: For a 0.1 M weak acid with Ka = 1.8 x 10-5: Initial: [HA] = 0.1 M Let x = [H+] produced Equilibrium: Ka = [H+][A-]/[HA] = (x)(x)/(0.1-x)
The Säure-Basen-Haushalt (acid-base balance) in biological systems relies heavily on these principles, particularly in maintaining blood pH and proper cellular function. Understanding these calculations helps in various fields, from environmental science to medical diagnostics.
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Improve your grades
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A buffer solution is a specialized mixture that maintains a stable pH when small amounts of acids or bases are added. This remarkable property makes buffers essential in biological systems and industrial processes where pH control is critical.
Definition: A buffer solution consists of a weak acid and its salt, or a weak base and its salt, working together through the common-ion effect to resist pH changes.
The buffer capacity represents how much acid or base a buffer can neutralize before significant pH changes occur. There are two main types of buffers:
Highlight: Buffer solutions are crucial in:
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The human body relies on several buffer systems to maintain precise pH levels. The pH scale, discovered by Søren Sørensen in 1909, helps measure these delicate acid-base balances.
Example: Blood pH must stay remarkably close to 7.4. Even small deviations can be dangerous:
Key biological buffer systems include:
Vocabulary: Ampholytes are molecules that can act as both acids and bases, making them excellent biological buffers.
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Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
The Henderson-Hasselbalch equation provides a mathematical framework for calculating buffer pH:
pH = pKa + log([base]/[acid])
This equation shows the relationship between:
Definition: The equation helps predict how buffer composition affects pH and can be used to design buffers with specific pH values.
For acid buffers: pH = pKa + log([salt]/[weak acid]) For base buffers: pOH = pKa + log([salt]/[base])
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Buffer solutions find extensive use across multiple fields:
Example: A common buffer preparation involves mixing 1.0M acetic acid with 1.0M sodium acetate to create a buffer with pH 4.76, which remains stable even when small amounts of acid or base are added.
Access to all documents
Improve your grades
Join milions of students
By signing up you accept Terms of Service and Privacy Policy
The Brønsted-Lowry concept fundamentally transformed our understanding of acid-base chemistry by focusing on proton transfer reactions. In this framework, acids and bases are defined by their behavior during chemical reactions rather than just their properties in isolation. An acid serves as a proton donor, while a base acts as a proton acceptor, creating a dynamic relationship that underlies countless chemical processes.
Definition: A conjugate acid-base pair consists of two chemical species that differ by exactly one proton (H+). When an acid donates its proton, it becomes its conjugate base. Similarly, when a base accepts a proton, it becomes its conjugate acid.
The relationship between acids and bases extends beyond simple proton transfer. Ampholytes are species that can act as either acids or bases depending on the reaction conditions, demonstrating the contextual nature of acid-base behavior. This concept is crucial for understanding biological systems, where many molecules must maintain precise pH balance through amphoteric behavior.
The solubility product principle represents a specialized application of chemical equilibrium laws to heterogeneous systems. This principle specifically addresses situations involving slightly soluble electrolytes and their saturated solutions. When a solid ionic compound dissolves in water, it establishes an equilibrium between the solid phase and its ions in solution. The mathematical expression of this equilibrium, known as the solubility product constant (Ksp), provides a quantitative measure of solubility.
Example: Consider silver chloride (AgCl) dissolving in water: AgCl(s) ⇌ Ag+(aq) + Cl-(aq) The solubility product expression would be: Ksp = [Ag+][Cl-]
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Improve your grades
Join milions of students
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The concept of pH, developed by Soren Sorensen in 1909, revolutionized our understanding of acid-base chemistry. The pH scale provides a logarithmic measure of hydrogen ion concentration in aqueous solutions, ranging from 0 to 14. This scale is fundamental to chemistry, biology, and numerous industrial applications.
Vocabulary: The Ionenprodukt des Wassers (ion product of water) represents the equilibrium constant for water's self-ionization, written as Kw = [H+][OH-] = 1.0 × 10^-14 at 25°C.
Understanding the relationship between pH and concentration is crucial for various applications. The logarithmic nature of the pH scale means that each unit change represents a tenfold difference in hydrogen ion concentration. This mathematical relationship helps explain why small changes in pH can have significant effects in biological systems and chemical processes.
The concept of Autoprotolyse (autoprotolysis) explains how water molecules can act as both acid and base, transferring protons between themselves to maintain equilibrium. This self-ionization of water establishes the foundation for understanding acid-base behavior in aqueous solutions and helps explain why pure water has a pH of 7 at room temperature.
Highlight: The pH scale's logarithmic nature means that a solution with pH 4 is ten times more acidic than a solution with pH 5, and one hundred times more acidic than a solution with pH 6.
Our AI companion is specifically built for the needs of students. Based on the millions of content pieces we have on the platform we can provide truly meaningful and relevant answers to students. But its not only about answers, the companion is even more about guiding students through their daily learning challenges, with personalised study plans, quizzes or content pieces in the chat and 100% personalisation based on the students skills and developments.
You can download the app in the Google Play Store and in the Apple App Store.
That's right! Enjoy free access to study content, connect with fellow students, and get instant help – all at your fingertips.
App Store
Google Play
The app is very easy to use and well designed. I have found everything I was looking for so far and have been able to learn a lot from the presentations! I will definitely use the app for a class assignment! And of course it also helps a lot as an inspiration.
Stefan S
iOS user
This app is really great. There are so many study notes and help [...]. My problem subject is French, for example, and the app has so many options for help. Thanks to this app, I have improved my French. I would recommend it to anyone.
Samantha Klich
Android user
Wow, I am really amazed. I just tried the app because I've seen it advertised many times and was absolutely stunned. This app is THE HELP you want for school and above all, it offers so many things, such as workouts and fact sheets, which have been VERY helpful to me personally.
Anna
iOS user
I think it’s very much worth it and you’ll end up using it a lot once you get the hang of it and even after looking at others notes you can still ask your Artificial intelligence buddy the question and ask to simplify it if you still don’t get it!!! In the end I think it’s worth it 😊👍 ⚠️Also DID I MENTION ITS FREEE YOU DON’T HAVE TO PAY FOR ANYTHING AND STILL GET YOUR GRADES IN PERFECTLY❗️❗️⚠️
Thomas R
iOS user
Knowunity is the BEST app I’ve used in a minute. This is not an ai review or anything this is genuinely coming from a 7th grade student (I know 2011 im young) but dude this app is a 10/10 i have maintained a 3.8 gpa and have plenty of time for gaming. I love it and my mom is just happy I got good grades
Brad T
Android user
Not only did it help me find the answer but it also showed me alternative ways to solve it. I was horrible in math and science but now I have an a in both subjects. Thanks for the help🤍🤍
David K
iOS user
The app's just great! All I have to do is enter the topic in the search bar and I get the response real fast. I don't have to watch 10 YouTube videos to understand something, so I'm saving my time. Highly recommended!
Sudenaz Ocak
Android user
In school I was really bad at maths but thanks to the app, I am doing better now. I am so grateful that you made the app.
Greenlight Bonnie
Android user
I found this app a couple years ago and it has only gotten better since then. I really love it because it can help with written questions and photo questions. Also, it can find study guides that other people have made as well as flashcard sets and practice tests. The free version is also amazing for students who might not be able to afford it. Would 100% recommend
Aubrey
iOS user
Best app if you're in Highschool or Junior high. I have been using this app for 2 school years and it's the best, it's good if you don't have anyone to help you with school work.😋🩷🎀
Marco B
iOS user
THE QUIZES AND FLASHCARDS ARE SO USEFUL AND I LOVE THE SCHOOLGPT. IT ALSO IS LITREALLY LIKE CHATGPT BUT SMARTER!! HELPED ME WITH MY MASCARA PROBLEMS TOO!! AS WELL AS MY REAL SUBJECTS ! DUHHH 😍😁😲🤑💗✨🎀😮
Elisha
iOS user
This app is phenomenal down to the correct info and the various topics you can study! I greatly recommend it for people who struggle with procrastination and those who need homework help. It has been perfectly accurate for world 1 history as far as I’ve seen! Geometry too!
Paul T
iOS user
The app is very easy to use and well designed. I have found everything I was looking for so far and have been able to learn a lot from the presentations! I will definitely use the app for a class assignment! And of course it also helps a lot as an inspiration.
Stefan S
iOS user
This app is really great. There are so many study notes and help [...]. My problem subject is French, for example, and the app has so many options for help. Thanks to this app, I have improved my French. I would recommend it to anyone.
Samantha Klich
Android user
Wow, I am really amazed. I just tried the app because I've seen it advertised many times and was absolutely stunned. This app is THE HELP you want for school and above all, it offers so many things, such as workouts and fact sheets, which have been VERY helpful to me personally.
Anna
iOS user
I think it’s very much worth it and you’ll end up using it a lot once you get the hang of it and even after looking at others notes you can still ask your Artificial intelligence buddy the question and ask to simplify it if you still don’t get it!!! In the end I think it’s worth it 😊👍 ⚠️Also DID I MENTION ITS FREEE YOU DON’T HAVE TO PAY FOR ANYTHING AND STILL GET YOUR GRADES IN PERFECTLY❗️❗️⚠️
Thomas R
iOS user
Knowunity is the BEST app I’ve used in a minute. This is not an ai review or anything this is genuinely coming from a 7th grade student (I know 2011 im young) but dude this app is a 10/10 i have maintained a 3.8 gpa and have plenty of time for gaming. I love it and my mom is just happy I got good grades
Brad T
Android user
Not only did it help me find the answer but it also showed me alternative ways to solve it. I was horrible in math and science but now I have an a in both subjects. Thanks for the help🤍🤍
David K
iOS user
The app's just great! All I have to do is enter the topic in the search bar and I get the response real fast. I don't have to watch 10 YouTube videos to understand something, so I'm saving my time. Highly recommended!
Sudenaz Ocak
Android user
In school I was really bad at maths but thanks to the app, I am doing better now. I am so grateful that you made the app.
Greenlight Bonnie
Android user
I found this app a couple years ago and it has only gotten better since then. I really love it because it can help with written questions and photo questions. Also, it can find study guides that other people have made as well as flashcard sets and practice tests. The free version is also amazing for students who might not be able to afford it. Would 100% recommend
Aubrey
iOS user
Best app if you're in Highschool or Junior high. I have been using this app for 2 school years and it's the best, it's good if you don't have anyone to help you with school work.😋🩷🎀
Marco B
iOS user
THE QUIZES AND FLASHCARDS ARE SO USEFUL AND I LOVE THE SCHOOLGPT. IT ALSO IS LITREALLY LIKE CHATGPT BUT SMARTER!! HELPED ME WITH MY MASCARA PROBLEMS TOO!! AS WELL AS MY REAL SUBJECTS ! DUHHH 😍😁😲🤑💗✨🎀😮
Elisha
iOS user
This app is phenomenal down to the correct info and the various topics you can study! I greatly recommend it for people who struggle with procrastination and those who need homework help. It has been perfectly accurate for world 1 history as far as I’ve seen! Geometry too!
Paul T
iOS user