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carminetiger314Lv1

28 Nov 2020

Are given some acids and Ka vales:

HClO₄ → Ka= 1 x 10⁷

HOAc → Ka= 1.76 x 10^-5

HCN → Ka= 4.93 x 10^-10

HF → 3.53 x 10^-4

What is the order of increasing base strength?

a. CN^-, ClO₄^-, F^-, OAc^-

b. ClO₄^-, OAc^-, CN^-, F^-

c. CN^-, F^-, OAc^-, ClO₄^-

d. ClO₄^-, F^-, OAc^-,CN^-

e. CN^-, OAc^-, F^-, ClO₄^-

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Related questions

Which of the following acids, (listed with Ka values), and their conjugate base will form a buffer with a pH of 2.34?

Please, show calculations:

A) HF, K_a = 3.5 x 10 ^-4

B) HClO, K_a = 2.9 x 10 ^-8

C) HC₇H₅O₂ K_a = 6.5 x 10 ^-5

D) HCN, K_a = 4.9 x 10 ^-10

E) HClO₂, K_a = 1.1 x 10 ^-2

please answer all parts!! running out of time!

a) You will be titrating a 1.50 M solution of HCN. What is the initial pH of this solution before the titration has begun? b) We measure out 21.00 mL of a 1.50 M solution of HCN for our titration with sodium hydroxide. If you add 1.00 mL of a 0.30 M solution of sodium hydroxide, what is the pH of the acid solution at this stage of the titration? The Ka for HCN is 4.9 x 10-10 1.00 mL of sodium hydroxide added to the weak acid 0.30M sodium hydroxide in the buret as the titrant 21.0 mL of original 1.50 M HCN sample c) If we add enough sodium hydroxide to neutralize 1/2 of our HCN, we will have converted 1/2 the HCN into CN. At this point the [HCN] = [CNT, what is the pH at this point that we call the half equivalence point? d) If we add enough sodium hydroxide to neutralize all of the HCN, we will convert it all into CN and we will have reached the equlvalence point. Since the only thing that remains at the equivalence point is the salt of the conjugate base, CN, the pH at equence will be determined by the hydrolysis of this salt. Since you know how many moles of HCN you started with, you know how many moles of CN must be present at the equivalence point. To calculate the [CN ] you must know the total volume at the equivalence point. How many mL of 0.30 M sodium hydroxide are needed to reach the endpoint? e) What is the pH at the equivalence point of this titration? Remember that since the conjugate base, CN, is hydrolyzing in solution, you will need a Kb value for this base f) If we pass the equivalence point then the pH of the solution is dominated by the strong base. It is like a limiting reagent problem where now, we have run out of the weak acid and there is excess strong base. Even though there will be CN in solution, the OH from the strong base will control the pH. Thus, it is like a strong base pH problem. If we add 115.00 mL of sodium hydroxide we will be well past the equivalence point of the titration. What will be the pH at this point. (Hint: how much strong base will remain unreacted in solution?)

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