## Bronsted-Lowry Acid-Base Reaction **Objective:**Using the Bronsted-Lowry model, write an equation to show why the following species produce a basic aqueous solution.**Instructions:**Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.### Equation\[ \text{HS}^- (aq) + \text{H}_2\text{O} (l) \rightarrow \_\_\_\_ + \_\_\_\_ \]### Interactive Elements:- **Submit Answer**- **Try Another Version**### Additional Information:- You have 4 item attempts remaining.**Note:** Ensure you write the balanced chemical equation correctly and include the phases (states) of each species involved.---**Explanation of Elements on the Page:**1. **Text Box Areas:** Two blank boxes where you are supposed to input the resulting species from the reaction. Make sure to input both the product and the byproduct of the reaction.2. **Submit Answer Button:** A button to submit your written equation for validation.3. **Try Another Version Button:** An option to attempt the problem again if needed.4. **Item Attempts Remaining:** Indicates how many more times you can try to submit your answer.**No Graphs or Diagrams provided in this content.**

According to bronsted lowry Acid is a species which can donate H^+ and base is species which can…

13.1-13.3) [References] Using the Bronsted-Lowry model, write an equation to show why the following species produce a basic aqueous solution. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank) HS (aq) + H20(1)

13.1-13.3) [References] Using the Bronsted-Lowry model, write an equation to show why the following species produce a basic aqueous solution. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank) HS (aq) + H20(1)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

9:10 2- 3C₂²- + Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. Be sure to include the proper phases for all species within the reaction. C (CH3)2NH2CIO, 1 2 3 4 (s) Question 7 of 12 O CI Reset LO H₂O 5 1 6 7 8 6 H Submit 个 Tap here or pull up for additional resources 9 11 N OH- NR H3O+ (aq) O x H₂O
The most common source of acidity in water is dissolved carbon dioxide, CO2. Using the Brønsted-Lowry concept, show how CO2 yields hydronium ion in aqueous solution without involving the species H2 CO3. (Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank. Use H30* for hydronium ion.)
Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. Be sure to include the proper phases for all species within the reaction. (CH₃)₂NH₂ClO₄
9:49 2- 3C₂²- + Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. Be sure to include the proper phases for all species within the reaction. (CH3)3NHBr 1 2 3 4 C (s) Question 9 of 11 H3O+ Reset LO 5 6 O H₂O OH- NR 6 7 8 9 Br Tap here or pull up for additional resources Submit 个 H 10 (aq) ( O N x H₂O
A) Please fill in the first blank with the word "acidic", "basic" or "nearly neutral". B) SHOW ALL WORK FOR THE pH QUESTION. WRITE YOUR FINAL NUMERICAL RESPONSE IN THE SPACE PROVIDED BELOW. Hint: IF you need Ka to solve this problem, you must calculate it from the information provided below. When 0.77 M ammonium chloride salt hydrolyzes in water, the solution will be with a pH = Kb (NH3) = 1.8 x 105 %3D
1 The base protonation constant K, of 1-H-imidazole (C,H,N,) is 9.0 x 10 °. Calculate the pH of a 1.1 M solution of 1-H-imidazole at 25 °C. Round your answer to 1 decimal place. pH =| Continue Terms of Use 2022 McGraw Hill LLC. All Rights Reserved.
a) Carbonic acid (H,CO;) is a weak diprotic acid. Write expressions for Kj and K, of H,CO,. Note that you are not required to write dissociation reactions, but expressions, i.e. K,l =.... and K,2 = .. a. 2 b) Say whether each of the following solutions is acidic, basic or neutral. b. 2 i) 10 3 МОН ii) 10 * M H,O*
Indicate whether following reactions is a strong, weak, or nonelectrolyte represented in the following equations: 1) C6H12O6(s) (in H2O) --> C6H12O6(aq) 2) MgCl2(s) (in H2O) --> Mg2+(aq) + 2Cl-(aq)
help please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working
How many moles of B (weak base) would need to be added to 524 mL of 0.209 M BHCl (the acidic salt) to produce a solution with a pH equal to 9.02? Report your answer to the thousandths place. The Kb of the weak base (B) is 3.8 × 10-6.
At 22 °C, an excess amount of a generic metal hydroxide, M(OH)2, is mixed with pure water. The resulting equilibrium solution has a pH of 10.20. What is the Ksp of the salt at 22 °C? Give detailed Solution..don't give Handwritten answer