What is the pH of a 1.0 L solution that is 0.50 M PO43- and 0.50 M HPO42-? (The pKa values for H3PO4are: 2.14, 7.2, and 12.4 respectively) If 0.01 moles of OH- is added to the above buffer, what will the new pH be? Change of volume is negligible. If 0.01 moles of OH- is added to 1.0 L of water, what will the new pH be? Change of volume is negligible.

A buffer solution is 0.366 M in HF and 0.372 M in KF . If Ka for HF is 7.2×10-4 , what is the pH of this buffer solution? --- A buffer solution is 0.485 M in NAHS and 0.336 M in . If ka1  for H2S is , what is the pH of this buffer solution? pH =

A buffer solution is 0.416 M in H2 S and 0.245 M in NaHS. If K21 for H2S is 1.0 x 10-7, what is the pH of this buffer solution? pH =| A buffer solution is 0.376 M in N.HSO3 and 0.390 M in Na,SOg. If K, for HSO3 is 6.4 × 10-8, what is the pH of this buffer solution? pH =

When a solution is titrated with an base, an indicator (HIn) changes from yellow to blue (In). The Ka of the indicator is 8.00e - 06. At what pH will the indicator color change first be visible? pH = 6.0969 X 0%

5:48 PM Wed Nov 16 Today 5:48 PM 目。 oint when 15.0 ml. of o. 75% Calculate the pH of a titration at the point when 15.0 mL of 0.15 M NaOH is added to 30.0 mL of 0.20 M HNO3 Edit G ¯¯¯

The pH of unbuffered water, such as rain, is decreasing consistently over time as atmospheric CO2 concentrations increase. a) What will be the atmospheric CO2 level (in ppm) when the pH of rain water reaches 5.50 at 25 °C? b) What would be the pH of buffered water (over CaCO3 limestone at 25 °C) at the CO2 level in part a)? c) Determine the concentrations of HCO3– and CO32– ions in the buffered water of part b) and then determine the alkalinity of the solution in ppm CaCO3.

10. One characteristic of blood that we rarely give a thought to is its pH. The pH of blood must be held remarkably constant, varying only by a few hundredths of a pH unit from 7.36 to 7.40.  Blood pH is kept constant primarily through the buffering action of the bicarbonate ion, HCO3-, and dissolved carbon dioxide, commonly represented as H2CO3. The second ionization is negligible in blood so that H2CO3 can be treated as a monoprotic acid.  A) If the Ka1 for H2CO3 is 4.2 * 10-7, what ratio of HCO3- to H2CO3 is necessary to produce a buffer of pH 7.40? B) What is the pH of a buffer that is 1.0 M NaHCO3 and 1.0 M H2CO3? C) If you have 1.00 L of the buffer described above (1.0 M NaHCO3 and 1.0 M H2CO3) and 10.0 mL of 0.100 M HCl is added to it, what is the new pH? D) Just to prove that the buffer helps minimize changes in pH, calculate the pH of a solution prepared by adding 10.0 mL of 0.1 M HCl to 1.00 L of pure water.

A 1.47 L buffer solution consists of 0.173 M butanoic acid and 0.299 M sodium butanoate. Calculate the pH of the solution following the addition of 0.060 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The K, of butanoic acid is 1.52 x 10-. pH =

It's 0.1 ml of 1 M HCl

What will be the resulting pH if we add 0.010 mole of HCl to 1 L of the acetate buffer solution in the previous example? 0.10 M CH3COOH, 0.15 M CH3COO-, pH = 4.92, pKa = 4.74(HINT: the pH should decrease but only slightly)