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Chemistry
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13 Dec 2019

True or False


a) a strong acid solution will always have a lower pH than aweak acid solution


b) For solutions of equal concentration, the pH of weak acidsolution (Ka1) will be lower than that of second weak solution(Ka2) only if Ka1<Ka2


c) For solutions of equal concentrations, the pH of a strongacid solution will always be less than that of a weak acidsolution.

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Casey Durgan
Casey DurganLv2
17 Dec 2019

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Related questions

Tartaric acid is a weak diprotic fruit acid with Ka1 = 1.0 x 10-3 and Ka2 = 4.6 x 10-5.

(a) Letting the symbol H2A represent tartaric acid, write the chemical equations that represent Ka1 and Ka2. Write the chemical equation that represents Ka1 x Ka2.

(b) Qualitatively describe the concentrations of H2A, HA-, A2-, and H3O+ in a solution that is about 0.5 M in tartaric acid. 

(c) Calculate the pH of a 0.0250 M tartaric acid solution and the equilibrium concentration of [H2A].

(d) What is the A2- concentration in solutions b and c. 

For the diprotic weak acid H2A, Ka1 = 3.4 × 10-6 and Ka2 = 5.5 × 10-9. What is the pH of a 0.0700 M solution of H2A? What are the equilibrium concentrations of H2A and A2– in this solution? Express Ka1 in terms of x, and then show the simplified expression (when x is assumed to be negligible compared to to the initial concentration). Also, give the numerical value of x using the appropriate approximation. What is the pH of the solution if you stopped here?

1.) What is the definition of a strong acid compared to that of aweak acid?

2.) Is it possible to have a pH for a weak acid that is lower thana pH for a strong acid (of different concentrations), why or whynot?

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