Question

QUESTIONS 1. Consider the buffer mixture that you created in Part C.1 of the procedure. a. How many moles of NaC,H,O, are con
b. HCO,H c. 50:50 mixture of HCO,H + NaHCO, d. (CH) NHẠC e. 50:50 mixture of (CH),NH + ((CH), NH,)CI f. 50:50 mixture of 0.1


C. pH of Buffer Solutions In the unshaded portions of the following table, supply the calculated molarities of the indicated
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Answer #1

Question 2.

Part a.

KCl is neutral.

Explanation: KCl is formed by the combination of a strong acid (HCl) with a strong base (KOH). Hence, the salt doesn't undergo hydrolysis.

Part b.

HCO2H is acidic.

Explanation: HCOOH is a weak acid with Ka = 1.8*10-4.

Part c.

50:50 mixture of HCO2H + NaHCO2 is acidic.

Explanation: This is a buffer solution, where the pH = pKa = 3.74.

Part d.

(CH3)2NH2Cl is acidic.

Explanation: The salt dissociates into a strong conjugate acid.

Part e.

50:50 mixture of (CH3)2NH + (CH3)2NH2Cl is basic.

Explanation: This is a buffer solution, where the pH = pKa = 10.73.

Part f.

50:50 mixture of 0.1 M NaNO3 + 0.1 M HNO3 is acidic.

Explanation: The solution has the pH = -Log(0.1) = 1

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