Choose the compound (or compounds) that best match the descriptions.1. NaCIO,Superacid2. H2SO4 and H3PO4Lewis acid, not a Bronsted-3. BeF2Lowry acid4. CH3NH3CIMakes a buffer with HCIO,5. CIO4Makes a buffer withCH3NH3Br6. CH3NH2Lewis base, not a Bronsted-Lowry base7. HCIO48. B(OH)3 and HCIO4

Superacid HClO4 Lewis acid, not a Bronsted Lowry acid BeF2 is the Lewis acid since it can accept…

Answered: 4. CH3NH3CI Makes a buffer with HCIO,…

4. CH3NH3CI Makes a buffer with HCIO, 5. CIO4 Makes a buffer with CH3NH3B 6. CH3NH2 Lewis base, not a Bronsted- Lowry base 7. HCIO4 8. B(OH)3 and HCIO <> > >

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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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

Choose the compound (or compounds) that best match the descriptions.
1. NaCIO,
Superacid
2. H2SO4 and H3PO4
Lewis acid, not a Bronsted-
3. BeF2
Lowry acid
4. CH3NH3CI
Makes a buffer with HCIO,
5. CIO4
Makes a buffer with
CH3NH3Br
6. CH3NH2
Lewis base, not a Bronsted-
Lowry base
7. HCIO4
8. B(OH)3 and HCIO4

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Calculate the pH of a buffer solution made by dissolving 50 g of NaHCO3 and 20 g of H2CO3 to make 100 mL of a buffer solution. Help! H2CO3 Ka1= 4.30 x 10^-7 a. 6.77 b. 6.63 c. 6.10 d. 6.37
You have two buffered solutions. Buffered solution 1 consists of 5.0 M HOAc and 5.0 M NaOAc; buffered solution 2 is made of 0.050 M HOAc and 0.050 M NaOAc. How do the pHs of the buffered solutions compare? Select one: a. The pH of buffered solution 1 is greater than that of buffered solution 2. b. The pH of buffered solution 2 is greater than that of buffered solution 1. c. The pH of buffered solution 1 is equal to that of buffered solution 2. d. Cannot be determined without the Ka values. e. None of these (A-D).
7. Consider a buffered solution at a pH of 4.00 made with HF (K₁ = 7.2 x 104) and NaF. Which of the following statements is true? Assume all of the concentrations below refer to equilibrium concentrations. A) [HF] = [F] B) [HF] = [H*] C) [HF] > [F] qme D. [H¹] = [F] E. [HF] [F]
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