Calculate the pH of a solution that is prepared by dissolving 0.174 mol of m-chlorobenzoic acid (C6H4CICOOH, K, 1.00x104) and 0.430 mol of hydrocyanic acid (HCN, K, 6.17x10-10) in water and diluting to 2.40 L. Also, calculate the equilibrium concentrations of CeHaCICOOH, C6H4CICOO, HCN, and CN". Do not make an approximation unless the initial acid concentration is greater than 1000 x Ka. (Hint: The pH will be determined by the stronger acid of this pair.) pH = [C6H4CICOOH) = [CH₂CICOO"]= [HCN] = [CN"]= M M M M

Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5. Values of K, for Some Common Weak Bases Conjugate Name Formula Acid Kb Ammonia NH3 NH4+ 1.8 x 10-5 Methylamine CH3NH2 CH3NH3 + 4.38 x 10-4 Ethylamine C₂H5NH₂ C₂H5NH3+ 5.6 x 10-4 Aniline C6H5NH3 + 3.8 x 10-10 CH;NH, C,H,N Pyridine CH;NH* 1.7 x 10-⁹ 1. Compute the poH of the buffer solution. (Supply answer up to the 1st decimal point)

Calculate the pH of an acetic acid solution, originally 0.25 M, in water. The pKa for acetic acid = 4.76.

Calculate the pH and fraction of dissociation (?) for each of the acetic acid (CH3COOH, p?a=4.756) solutions. A 2.15*10^-12 M solution of CH3COOHCH3COOH.

What is the pH of the solution that is prepared by dissolving 0.8 g of lactic acid (90,08 g/mol, Ka - 1.4 x 10) and 1.3g of sodium lactate (112.06 g/mol) in water and diluted to 1.00 L? Round your caiculated value for pH to two figures to the right of the decimal point.

A 1.384 g sample of N-2-acetamido-2-aminoethane-sulfonic acid potassium salt (ACES K+, MW = 220.29 g/mol) dissolved in 60.62 mL of water.To the solution, 29.89 mL of HCl is added, resulting in a pH of 6.50. Calculate the concentration of the HCl solution. The pKa of ACES is 6.85. [HCI] .072 M

An analytical chemist is titrating 92.3 mL of a 0.6600M solution of ethylamine (C₂H5NH₂) with a 0.2000M solution of HNO3. The pK, of ethylamine is 3.19. Calculate the pH of the base solution after the chemist has added 83.0 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. PH 7 X Ś ? C ol Ar

Isobutylamine is a weak base. If the initial concentration of isobutylamine is 0.055 M and teh equilibrium concentration of OH is 4.0 x 10 -3 M, calculate Kb for isobutylamine.

A 1.819 g sample of N-2-acetamido-2-aminoethane-sulfonic acid potassium salt (ACES-K+, MW = 220.29 g/mol) is dissolved in 91.44 mL of water. To the solution, 16.99 mL of HCl is added, resulting in a pH of 6.72. Calculate the concentration of the HCI solution. The pKa of ACES is 6.85. [HC1] 0.328 Incorrect M

Using the literature value (from Kotz et al) for the Ka for HC3H5O2 (propanoic acid, also written as C2H5CO2H), calculate the theoretical Kb for the C3H5O2- propionate ion and the theoretical pH of a 0.173 M solution of sodium propionate. Using the literature Ka for theCH3NH3+ ion, calculate the theoretical pH of a 0.147 M solution of methylammonium chloride. What is the hydroxide ion concentration? A 0.119 M solution of Covidenol, a weak acid, has a measured pH of 3.45.  Determine the pKa of Covidenol.