Which of the following yields a buffer solution when equal volumes of the two so

Question

Which of the following yields a buffer solution when equal volumes of the two solutions are mixed? 0.10 M H_2C0_3 and 0.050 M HCl 0.10 M H_2CO_3 and 0.10 M KOH 0.10 M H_2CO_3 and 0.10 M HCl 0.10 M H_2CO_3 and 0.050 M KOH 0.10 M K_2CO_3 and 0.050 M KOH Calculate the pH of a 1.6 M KOH solution. 1.60 - 0.20 0.20 14.20 13.80 You have 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH_3COOH) and 0.30 M sodium acetate (CH_3COOH What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? K_a = 1.8 times 10^-5. 4.41 4.74 4.56 4.92 5.07 Which of the following solutions is basic? [OH^-] = 1.0 times 10^-14 M [OH^-] = 1.0 times 10^-7M. [H_3O^+] = 1.0 times 10^-14 M [H_3O^+] > 1.0 times 10^-7 M [H^-]

Explanation / Answer

10.

buffer is nothing but a combination of week acid and week base

both concentrations should not be equal

H2CO3 HCl both are acids so with these we cant make the buffer

so option A, option C and option E are not a buffer solutions

in option B both are in 1:1 ratio

option D is correct answer.

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