Calculate the pH of each solution.A solution containing 0.0313 M maleic acid and 0.044 M disodium maleate. The K₂ values for maleic acid are1.20 x 10-² (K₁1) and 5.37 x 10-7 (K₁2).pH7.67PHIncorrectA solution containing 0.0353 M succinic acid and 0.023 M potassium hydrogen succinate. The K₂ values for succinic acid are6.21 x 10-5 (K₁1) and 2.31 x 10-6 (K₁2).5.36Incorrect

ANSWER-1The pH for the maleic acid and disodium maleate solution is approximately 2.07.ANSWER-2The…

Answered: Calculate the pH of each solution. A…

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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< Which of the following solutions would be expected to have a pH of 7.00? Weak Acid HCN HNO₂ HIO HBrO C6H5COOH Ka 4.9 x 10-1⁰ 4.5 x 10-4 2.3 x 10-¹1 2.5 x 10-⁹ 6.3 x 10-5 Question 4 of 11 Tap here or pull up for additional resources Weak Base HONH, NH3 CoHsNH, H₂NNH₂ C5H5N A) CSIO B) NaF C) LICIO3 D) KNO₂ Submit
3.
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Which of the following statements is TRUE? Select one: A solution with a pOH of 4 is basic. It is not possible to have a pH outside the range 0 - 14. A 1 M solution of HCl will have a higher pH than a 1 M solution of HF. Carbonic acid (Ka = 4.3 × 10-7) is a stronger acid than oxalic acid (Ka = 5.9 × 10-2). Basic solutions don't contain any H3O+ ions.
Calculate the pH and fraction of dissociation (a) for each of the acetic acid (CH COOH, pka = 4.756) solutions. A 0.00333 M solution of CH, COOH. A 2.15 x 10-12 M solution of CH, COOH. pH = 1 228 X10-7
Each solution below has pH = 4.5. Which solution most effectively maintains pH between 4.0 and 5.0 upon addition of a small amount of strong acid or base? O 1.00 M NaF +0.050 M HF. K₂(HF) = 6.3 x 10-4 O 2.1 M NaH₂PO4 + 0.0085 M H3PO4. Ka1(H3PO4) = 7.5 × 10-³ 0.80 M NaNO₂ + 0.055 M HNO₂. Ka(HNO2, nitrous acid) = 4.6 x 10-4 O 1.0 M NaC7H502 +0.50 M HC7H5O2. Ka(HC₂H5O₂, benzoic acid) = 6.3 × 10-5
h To add an 0 atom in basic solution, add 2 OH" to the side that needs the O atom, and also add an H20 to the other side. (OH has one more O than HOH). How many H20 molecules should be added to the left side? How many OH ions should be added to the right? H20 + CIO3 - CI" + OH Number of H50 molecules = 1 Number of OH ions =2
None
Hydrochloric acid is a strong acid. In a 0.01M solution, what are the pH value and the concentration of hydroxide ion? Select one: a. pH = 0.01 [OH-] = 0.01 mol dm-3 b. pH = 2 [OH-] = 10-12 mol dm-3 c. pH = 2 [OH-] = 12 mol dm-3 d. pH = 0.01 [OH-] = 12 mol dm-3
< Which of the following 1.0 M solutions would have the highest pH? Weak Acid HCN HNO₂ HIO HBrO C6H5COOH Ka 4.9 x 10-1⁰ 4.5 x 10-4 2.3 x 10-¹1 2.5 x 10-⁹ 6.3 x 10-5 Question 5 of 11 Tap here or pull up for additional resources Weak Base HONH, NH3 CoHsNH, H₂NNH₂ C5H5N A) KCN B) C5H5NHCI C) NalO D) NH₂Br Submit
Use the following table to predict the best acid / base pair for the desired pH/pOH value:pH = 5.00What is the best acid AND base pair? Name Acid Base pKa Hydrochloric acid HCl Cl- -7.00 Phosphoric acid H3PO4 H2PO4- 2.12 Hydrofluoric acid HF F- 3.18 Lactic acid Lactic acid Lactate 3.85 Acetic acid CH3COOH CH3COO- 4.74 Carbonic acid H2CO3 HCO3- 6.36 Dihydrogen phosphate H2PO4- HPO42- 7.21 Ammonium NH4+ NH3 9.25 Hydrocyanic acid HCN CN- 9.31 Bicarbonate HCO3- CO32- 10.25 Methylammonium ion CH3NH3+ CH3NH2 10.62 Hydrogen phosphate HPO42- PO43- 12.38
Find the pH of each mixture of acids. 0.085 M in HFHF (Ka=6.8×10−4)(a=6.8×10−4) and 0.230 M in HC6H5OHC6H5O (Ka=1.3×10−10) 0.105 M in formic acid (Ka=1.8×10−4)(a=1.8×10−4) and 0.050 M in hypochlorous acid (Ka=2.9×10−8)

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