Find the pH for the following solutions if it contains: [d] 0.105 M urea, Ka = 0.67 [e] 0.027 M lactic acid, Ka = 1.38 x 10 - 4 [f] 0.105 M aniline, pKa = 4.60 [g] 0.10 M ascorbic acid, pKa = 4.10

5) Find the concentration of H30*(aq) in a 1.75 M solution of lactic acid, HC3H5O3, at 25°C. Ka= 1.38 x 10*. 6) Write the equilibrium expression for the ionization of HOI, and calculate the concentration of HOI(aq) in solution if [H3O*]=2.3 x 10° M and pKa = 10.7 at 25°C.

You have a buffer solution containing an acid, HA. The pKa of HA is 7.20 and its conjugate base is A- (assume HA is monoprotic). What is the pH of the solution when [HA] = [A- ]? = 7.20  What is the pH of the solution when you have 10x [HA] to [A- ]? What if you have 10x [A- ] to [HA]?

Find the pH of a solution containing 0.22 M alanine (NH2CH(CH3)COOH) (pKa1= 2.34, pKa2= 6.87)

What is the concentration of the lactate ion in a 1.00 M lactic acid solution given that the Ka of HCH3H5O3 is 1.38 x 10 4? 5.26 x 105 M 1.38 x 10-4 M 1.17 x 102 M 1.00 M 0.998 M

1a) Determine the pH of 0.035 M NaF (pKa = 3.1).   1b) Determine the pH of 0.055 M oxalic acid (H2C2O4; Ka1 = 5.6x10-2; Ka2 = 5.4x10-5).

What is the pH of a buffer solution that contains 0.245 M weak acid and 0.450 M of the conjugate base? The pKa for the acid is 5.53.

Calculate the pH of each of the following buffered solutions. Ka(HC, HgO,)= 1.8 × 10 5 1.0.19 M acetic acid/0.29 M sodium acetate pH = 2. 0.29 M acetic acid/0.19 M sodium acetate pH = 3. 0.060 M acetic acid/0.21 M sodium acetate pH = 4. 0.21 M acetic acid/0.060 M sodium acetate pH = Visited

Just as pH is the negative logarithm of [H3O+], pKa is the negative logarithm of Ka, - log Ka The Henderson-Hasselbalch equation is used to calculate the pH of buffer solutions: How many grams of dry NH4C1 need to be added to 2.00 L of a 0.600 mol L-' solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.80? Kh for ammonia is 1.8 × 10–5. pKa base] pH = pKa +log acid Express your answer to two significant figures and include the appropriate units. Notice that the pH of a buffer has a value close to the pKa of the acid, differing only by the logarithm of the concentration ratio [base]/[acid]. • View Available Hint(s) ? X•10n Value mass of NHẠCI = Units

If you mix 125.0  mL of 0.50 M CH3CO2H with 75.0 mL of 0.83 M NaOH, what is the pH of the resulting solution? Kb of CH3COO- = 5.6 x 10-10 , Ka of CH3COOH = 1.8 x 10-5