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What set of acid and base combinations below could be used to generate sodium iodide, NaI?

a. NaOH and HF

b. HIO3 and Na2CO3

c. Na2CO3 and HI

d. NaOH and HI

e. both c & d

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Alyssa Mae Remarim
Alyssa Mae RemarimLv10
14 Jan 2021

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Related questions

Below are some questions and their answers. I would appreciate it if someone could please explain to me step by step how to get these answers?

1) One buffering component of your blood is the phosphate system that maintains your blood pH at 7.4. The major species of the phosphate system at this pH are likely:a. H3PO4 and H2PO4– b. H2PO4– and HPO42– c. HPO42– and PO43– d. H3PO4, H2PO4– and HPO42– e. H3PO4 only
answer: H2PO4– and HPO42–

2)Which solution is most acidic (has the lowest pH)? a. 0.15M HClO4 b. 0.30M hydrofluoric acid (remember HF is a weak acid) c. 1.5M potassium nitrite d. 1.5M sodium dihydrogen phosphate (NaH2PO4)
answer: 0.15M HClO4

3) The conjugate base of HC2O4− is_________. answer: C2O42−

4) Which of the following will not produce a buffered solution? a. 100 mL of 0.1 M Na2CO3 and 50 mL of 0.1 M HCl b. 100 mL of 0.1 M NaHCO3 and 25 mL of 0.2 M HCl c. 100 mL of 0.1 M Na2CO3 and 75 mL of 0.2 M HCl d. 50 mL of 0.2 M Na2CO3 and 5 mL of 1.0 M HCl e. 100 mL of 0.1 M Na2CO3 and 50 mL of 0.1 M NaOH
Answer: e. 100 mL of 0.1 M Na2CO3 and 50 mL of 0.1 M NaOH

5) Which solution has a greater pH 0.25 M NaHSO3 or 0.38 M NaHSO3? a. 0.25 M NaHSO3 b. 0.38 M NaHSO3 c. the pH of both solutions are the same because sodium bisulfite is a salt and salts are neutral d. the pH of both solutions are the same because bisulfite is amphoteric and amphoteric salts are neutral e. the pH of both solutions are the same because bisulfite is amphoteric and the pH only depends upon the pKa values
answer: e. the pH of both solutions are the same because bisulfite is amphoteric and the pH only depends upon the pKa values

For questions 13-14, use the information provided below from the experiment Identification of an Unknown. The molecular masses and reactions are provided for you.

NaHCO3 KHCO3 Na2CO3 K2CO3 NaCl KCl

84.01 g/mol 100.12 g/mol 105.99 g/mol 138.21 g/mol 58.44 g/mol 74.55g/mol

2 NaHCO3 (s) Ã Na2CO3 (s) + H2O (g) + CO2 (g) (Reaction 1)

Na2CO3 (s) +2HCl (aq) Ã 2NaCl (s) + H2O (l) + CO2 (g) (Reaction 2)

13. Brad starts with 0.652 g of unknown. How much mass should he have after the first heating step if his unknown
was NaHCO3?

A. 0.411 g Na2CO3

B. 0.326 g Na2CO3

C. 0.822 g Na2CO3

D. 0.00402 g Na2CO3

14. If Brad has a final mass of 0.270 g at the end of the experiment (after the 2nd heating), what is his percent yield
of the final salt? (Assuming he starts with 0.652 g of NaHCO3).

A. 40%

B. 60%

C. 80%

D. 86%

15. What is the concentration of chloride ions in 50.0 mL of a 5.25 M solution of barium chloride?

A. 0.525 M Cl-

B. 1.05 M Cl-

C. 5.25 M Cl-

D. 10.5 M Cl-

Aqueous Solutions

16. Which of the following represents a correct precipitation reaction between sodium iodide and lead(IV) sulfate?

A. PbSO4 (aq) + NaI(aq) Ã PbI (aq) + NaSO4 (aq)

B. PbSO4 (aq) + NaI(aq) Ã PbI (s) + NaSO4 (aq)

C. Pb(SO4)2(aq) + NaI (aq) Ã PbI2 (s) + Na2SO4 (aq)

D. Pb(SO4)2(aq) + NaI (aq) Ã PbI2 (aq) + Na2SO4 (aq)

17. How many of the following salts would not form a precipitate in an aqueous solution?

A. one

B. two

C. three

D. four

18. What type of reaction is the following? CaCO3 + heat à CaO + CO2

A. Combination

B. Decomposition

C. Single Replacement

D. Combustion

19. Calculate the amount of copper recovered from an 85% yield if the theoretical yield is 0.25 g

A. 21 g

B. 3.4 g

C. 0.21 g

D. 0.34 g

20. Which of the following chemical species is the oxidizing agent in the reaction below?

Cu (s) + 4 HNO3 (aq) → Cu(NO3)2 (aq) + 2 NO2 (g) + 2 H2O (l)

A. Cu (s)

B. HNO3 (aq)

C. Cu(NO3)2 (aq)

D. NO2 (g)

10. Write a balanced equation for each of the following reactions:

a. KHCO3(s) + HCl(aq) Ã

b. Ca(s) + H2SO4(aq) Ã

c. H2SO4(aq) + Al(OH)3(s) Ã

d. Na2CO3(s) + H2SO4(aq) Ã

11. Write a balanced equation for the neutralization of each of the following:

a. H3PO4(aq) + NaOH(aq) Ã

b. HI(aq) + LiOH(aq) Ã

12. A solution of 0.162 M NaOH is used to neutralize 25.0 mL of H2SO4 solution. If 32.8 mL of the NaOH solution is required, what is the molarity of the H2SO4 solution?

2H2O(l) + Na2SO4(aq) Ã 2H2O(l) + Na2SO4(aq)

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