If a buffer solution is 0.240 M in a weak acid (Ka = 8.1 × 10-5) and 0.430 M in its conjugate base, what is the pH?

What is the pH of a solution prepared by combining 0.258 mol of a newly discovered weak acid (Ka = 1.3 x 10-4) with 0.156 mol of the salt containing its conjugate base in 1.4 L of water?

A solution is prepared at 25 °C that is initially 0.29M in chloroacetic acid (HCH,CICO,), a weak acid with K,=1.3 × 10 and 0.34M in sodium chloroacetate (NaCH,CICO,). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = 0 ?

If a buffer solution is 0.200 M in a weak base (Kp = 8.7 × 10-) and 0.520 M in its conjugate acid, what is the pH? pH =

If a buffer solution is 0.180 M in a weak acid (Ka = 1.7 × 10 − 5 ) and 0.600 M in its conjugate base, what is the pH?

a buffer solution is often encountered during the titration of aweak acid. In such a titration, there is a strong base (often sodium hydroxide, as in today’s lab)which is being added to the weak acid. When the strong base reacts with the weak acid, theresult is the conjugate base of the weak acid. It is essential that you not confuse these twobases during the discussion below, and that you write your report so that it is clear which baseyou are talking about. If the pH of the acid solution is monitored during the titration, a pHprofile like the one below can be plotted. For monoprotic acids it will be sigmoid in shape:The Henderson-Hasselbalch equation helps to make sense of this curve (the base referredto is the conjugate base of the weak acid).pH = pKa + log ([base]/[acid])If calculations are desired, two points are particularly important. The first, at the steepest pointof the graph, is the equivalence point. At that point the acid has been completely consumed bythe strong base…

A solution contains 0.295 M potassium hypochlorite and 0.299 M hypochlorous acid (Ka The pH of this solution is = 3.50 × 10-8).

A buffer solution is made such that the initial concentrations of lactic acid (HC3H5O3) and the lactate ion (C3H­O­-) are 0.600 M and 0.620 M, respectively. What is the resulting pH if 300.0 mL of 0.100 M potassium hydroxide is added to 0.600 L of the buffer solution? (The Ka of HC3H5O3 is 1.4 x 10-4.) Answer not in scientific notation

What is the pH of a buffer solution that is 0.21 M methylamine and 0.20 M methylammonium chloride? K, (methylamine) = 4.4 × 10-4

calculate the pH of a dilute solution that contains the molar ratio of sodium acetate to acetic acid ( pka 4.76) of 1:3