If 10.0 mL of glacial acetic acid (pure HC2₂H3O2; K₁ = 1.8 x 10-5) is diluted to 1.35 L with water, what is the pH of the resulting solution? The density of glacial acetic acid is 1.05 g/mL. Express your answer to two decimal places. ΠΙ ΑΣΦ 3 pH = ?

The pH of a 0.84 M solution of barbituric acid (HC₂H₂N₂O3) is measured to be 2.04. Calculate the acid dissociation constant K of barbituric acid. Be sure your answer has the correct number of significant digits. K = 0 a x10 × Ś

An aqueous solution of 0.045 M HA (pKa = 11.11) is prepared. What is the pH of this solution? Enter your answer, rounded to the correct number of significant figures, into the box below. If your answer is a decimal, put a 0 before the decimal point. Do not use scientific notation. pH = X Seti30 HOTHECLARE 4.00

Calculate the pH of an aqueous KOH solution that is made by dissolving 654 mg of solid KOH in enough distilled water to make 100.0 mL of solution. Assume room temperature conditions. Note: molar mass of KOH = 56.105 g/mol; Kw at 25 °C = 1.00 × 10-14 %3D %D 6.987 10.000 0.933 13.066

For the diprotic weak acid H2A, ?a1=3.6×10−6 and ?a2=8.5×10−9. What is the pH of a 0.0800 M solution of H2A? pH=     What are the equilibrium concentrations of H2A and A2− in this solution? [H2A]=   M [A2−]=[A2−]=

What is the pH of 0.65 M ethanolamine, HOCH2CH2NH2, (Kb = 3.2 x 10−5)? pH =

A solution is prepared at 25°C that is initially 0.17M in propanoic acid (HC2H5CO2), a weak acid with Ka=1.3x10^−5, and 0.13M in sodium propanoate (NaC2H5CO2). Calculate the pH of the solution.   Round your answer to 2 decimal places.

What is the pH of the resulting solution when 15.00 mL of 0.28 M HCO₂H (K₂ = 1.8x10-4) is titrated with 7.00 mL of 0.30 M KOH? Report your answer with the correct number of significant figures.