What is the approximate pH of a solution X that gives the following responses wi

Question

What is the approximate pH of a solution X that gives the following responses with the indicators shown? A) 4.8 - 6.0 B) 8.2 - 10.0 C) 3.2 - 4.4 D) 6.0 - 7.6 What is the pH of a 0.020 M HCIC_4 solution? A) 1.70 B) 12.30 C) 0.040 D) 0.020 What is the pH of a 0.020 M Ba(OH)_2 solution? A) 1.40 B) 12.30 C) 12.60 D) 1.70 What is the pH of a solution prepared by diluting 25.00 mL. of 0.10 M HCI with enough water to produce a total volume of 100.00 mL? A) 1.60 B) 3.20 C) 2.00 D) 1.00 What is the pH of a solution made by mixing 100.0 mL of 0.10 M HNO_3, 50.0 mL of 0.20 M HCI and 100.0 mL of water? Assume that the volumes are additive. (moles are additive, but not molarity: so first calc moles in each solution (M times V(in L); add these and divide by the combined volume of the two solutions mixed) A) 0.30 B) 1.10 C) l.00 D) 0.82 What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Ca(OH)_2 with 50.00 mL of 0 100 M NaOH? Assume that the volumes are additive. A) 13.25 B) 12.78 C) 12.95 D)12.67 What is the equilibrium constant expression (K_a) for the acid dissociation of nitrous add HNO_2? The equation of interest is HNO_2(aq)+ H_2O(l) H_3O+(aq) + NO_2-(aq). A) K_a = ([HNO_2])/([H_3O+][NO_2-]) B) K_a = ([H_3O+][NO_2-])/([HNO_2][H_2O]) C) K_a = ([HNO_2][H_2O])/([H_3O+][NO_2-]) D) K_a = ([H_3O+][NO_2])/([HNO_2]) Determine the acid dissociation constant for a 0.10 M acetic acid solution that has a pH of 2.87. Acetic acid is a weak monoprotic acid and the equilibrium equation of interest is A) 1.8 times 10^-6 B) 1.8 Times 10^-5 C) 1.3 times 10^-3 D) 1.3 times 10^-2

Explanation / Answer

Q17.

pH for X if indicators:

from first methyl orange, this must hav pH greater thn 4.4

methyl red, pH must be greater than 6

meromothymol blue, pH must be between 6-7.6

phenolphtalein, colorless, it must be less 8.2

the best gues is bromothymol blue range, 6-7.6

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