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*

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*

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...

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3. Sodium benzoate, Na[C6H5COO], is soluble in water and is commonly used as a food preservative. If 4.7 g of the salt is dissolved to make 500. mL of solution, of the solution? (Benzoic acid is the name of the conjugate acid). 4.7 what is the pH Ans: 2.28 x 10-6M; 8.36
4. A solution was prepared by dissolving 0.541 g of benzoic acid (HC,H5COO) in 100 mL of water. The pH was measured to be 2.78. What is the K, for benzoic acid?
1. A 0.36 M hydrocyanic acid (HCN) solution has a pH of 4.87. Give: (a) the balanced equation for the ionization of hydrocyanic acid; (b) K. of HCN; (c) % ionization of HCN. a. b.
1. Sort each of the following 0.1 M salt solutions into the appropriate category below: NaCH;C00, НCСІ, НCN, NaОН, NH, NaCN, KNO;, H2SO, NH.CI, H.SO,, NaHCO;, NasPO, and CH,COOН. Strong Acids Weak Acids Neutral Salts Weak Bases Strong Bases
||| = O ACIDS AND BASES Determining the strength of acids from a sketch Four solutions of an acid dissolved in water are sketched below, as if under a microscope so powerful individual atoms could be seen. The same volume of solution is shown in each sketch. Note: Rank the solutions by the strength of the dissolved acid. That is, select 1 under the solution of the strongest acid, 2 under the solution of the next strongest acid, and so on. = H₂O Solution 1 (Choose one) Explanation Solution 3 (Choose one) Check ▼ ▬▬▬▬▬ Solution 2 (Choose one) ▼ Solution 4 (Choose one) 0/5 X spv7Aqws 3 Allie © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessi
4. Consider an aqueous solution of 1.50 M NH4Br. (Kb for NH3 = 1.8 x 10¹5) a) Which ion is pH neutral?; b) Which ion acts as an acid? c) Write a single net ionic equation to show that the solution is acidic. d) Calculate the pH the solution.
When 25.0 mL of 0.200 M hydroiodic acid and 25.0 mL of 0.200 M ammonia are combined, the pH of the resulting solution will be : ..... fill in the blank 1A. Less than 7B. Equal to 7C. Greater than 7
... 2@ 48 TO Time left 0:24:03 Consider a solution initially containing 0.40 mol fluoride anion (F) and 0.30 mol of hydrogen fluoride (HF). If 0.40 mol of HCl are added to this solution, which of the following statements is/are FALSE? Addition of 0.40 mol of HCI will lover the pH of solution by 0.4 unit. O You'll essentially have a weak acid solution situation, with 0.7 mol HF at the end. O You will still have a buffer solution at the end, since you'll still have significant amounts of both weak base and conjugate weak acid. You will no longer have a buffer solution, since all of the buffer capacity was exhausted. The pH will have shifted to a lower pH.
Write the balanced NET IONIC equation for the reaction that occurs when nitric acid and sodium fluoride are combined. It is not necessary to include states such as (aq) or (s).please box ionic equation + + This reaction is classified as: . acid , base or neutralThe extent of this reaction is: . below 50, above 50, 50 or 100When 35.0 mL of 0.200 M nitric acid and 35.0 mL of 0.200 M sodium fluoride are combined, the pH of the resulting solution will be seven. greater than , equal to, or less than
4. The equations and constants for the dissociation of three different acids are given below. HCO3 = H+ + CO?- K. = 4.2 x 10–7 -8 H;PO, = H+ + HPO- K. = 6.2 x 10 HSO, = H+ + SO?- Ka = 1.3 x 10–2 a. From the systems above, identify the conjugate pari that is best for preparing a buffer with a pH. of7.2. Explain your choice. b. Explain briefly how you would prepare the buffer solution described in (a) with the conjugate pair you have chosen. c. If the concentrations of both the acid and the conjugate base you have chosen were doubled, how would the pH be affected? Explain how the capacity of the buffer is affected by this change in concentrations of acid and base.
3. A solution with a pH of 2.91 is prepared by dissolving 1 g. of benzoic acid, HC,H,O,, a weak acid, in 350 mL of water. What is K, of benzoic acid?
A www-awn.aleks.com/alekscgi/x/lsl.exe/1o_u-IgNslkr7j8P3jH-lijkF O SIMPLE REACTIONS Identifying acids and bases by their chemical formula Classify each chemical compound listed in the table below. type of compound (check all that apply) compound ionic molecular acid base KNO, HNO, MgF2 NaOH 口|口| □|□ 口|口