An unknown acid, HA, has a percent dissociation of 2.16%. If the initial concent

Question

An unknown acid, HA, has a percent dissociation of 2.16%. If the initial concentration of the acid is 0.084 M. what is the pH of the solution? A.1.08 B.11.26 C.2.74 D.1233 E.1.67 11.A solution is prepared by dissolving 1.5523 g of the salt (CH_3)_2NH_2Br (MW= 126.01) in enough water to make 350.00 mL of solution. Calculate the pH of the solution. A.2.36 B.11.64 C.6.09 D.12.19 E.7.91 12.Which of the following weak acids would be BEST to use to make a buffer of pH=2.90? A.lactic B.butanoic C.chloroacetic D.benzoic E.hypochlorous 13.What is the pH of 126382 mL of a 0.0000862 M HB1O_3 solution? A.4.06 B.4.96 C.9.94 D.3.74 E.the pH can't be calculated witheut the value of K_a 14.Consider a 1 L buffer solution containing 0.40 M HF and 0.60 M NaF. Which of the following changes would completely destroy the buffer. K_a=3. 5x 10^-6 for HF. A.adding 0.400 mol HF B.adding 0.600 mol of HCI C.adding 0.300 mol of HCI D.adding 0.600 mol of KF E.adding 0.200 mol of KOH 15.Which of the following titrations of acids with bases would give a neutral solution at the equivalence point? A.titrating N_aOH with acetic acid B.titrating formic acid with LiOH C.titrating ammonia with HCI D.titrating HBrO_4 with N_aOH E.titrating HNO_3 with HCI

Explanation / Answer

10)
dissociation, x = 2.16% of 0.084 M = 1.8144*10^-3 M

HA ----> H+ + A-
0.084 0 0 (initial)
0.084-x x x

so,
[H+] = 1.8144*10^-3 M

pH = -log [H+]
= -log (1.8144*10^-3)
= 2.74

Answer: 2.74

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