A) 5.23 (B) .59 C)2.41 D)-2.46 A)5.23 (B)y.59 C)2.41 D)-2.46 E)1.14 11. Be able

Question

A) 5.23 (B) .59 C)2.41 D)-2.46 A)5.23 (B)y.59 C)2.41 D)-2.46 E)1.14 11. Be able to approximate the pH of a mixture of acids (strong and weak or two wedk acids) Find the pH of a mixture that is 0.075 M in HNO; and 0.175 M in HC HsQ2 A))1.12 B) 1.52 C) 12.48 D) 12.88 -l0 -01s (2) Find the pH of a mixture that is 0.020 M in HBr and 0.015 M in HCIO A) 1.70 B) 1.82 0.020t 1.46 Bo sorg 3) Find the pH of a mixture that is 0.100 M in HCHO2 and 0.050 M in HCIO. Ka of HCHO2 is 1.8 × 10-4, Ka of HCIO is 2.9 × 10-8.) A) 1.00 B) 2.05 C) 2.37 D) 3.46 E) 4.42 D)3.46 E) 442 12. Be able to solve among pH. Kb and initial concentration for a weak base or pH and initia concentration for a strong base (1) What is the pH of a 0.015 M aqueous solution of barium hydroxide (Ba(OH)2)? A) 12.25 B) 1.82 C) 12.48 D) 1.52 E) 10.41 (2) A saturated aqueous solution of calcium hydroxide (Ca(OH)2) has a pH of 12.25. What is t Ca] of such a solution? A)5.6×10-13 B) 2.3 × 10-5 C) 0.018 D) 8.9 x 10-3 E) 0.035

Explanation / Answer

given data

HCHO2 = 0.100 M

HClO = 0.050 M

HCHO2 is the weak acid and HClO is the conjugate base

therefore the solution will buffer

We can calculate the ph of the solution using the Henderson equation

pH =pka + log ([Base]/[acid])

pka of the HCHO2 = 3.74

now lets put the values in the formula

pH= 3.74 + log [ 0.050 M/0.100 M]

pH= 3.74 + (-0.3010)

pH = 3.44

So, the best and nearest answer is (C)

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