An acid solution at an initial concentration of 0.015 M. the pH of the acid solution at equilibrium was determined to be 5.3. Determine the Ka value of the acid.

Enough of a monoprotic weak acid is dissolved in water to produce a 0.0158 M solution. The pH of the resulting solution is 2.30. Calculate the pKa for the acid. pKa

Enough of a monoprotic weak acid is dissolved in water to produce a 0.0179 M solution. The pH of the resulting solution is 2.50. Calculate the Ka for the acid.

Enough of a monoprotic acid is dissolved in water to produce a 1.55 M solution. The pH of the resulting solution is 2.58. Calculate the K, for the acid. Ka =

An analytical chemist is titrating 135.0 mL of a 0.06400M solution of piperidine (CH,NH) with a 0.4700M solution of HNO3. The pK, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 21.3 mL of the HNO 3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO 3 solution added. Round your answer to 2 decimal places. pH = 0 ×

A buffer solution is prepared by combining 0.898 moles of formic acid and 0.733 moles of sodium formate. What will the solution pH be if 0.274 moles of sodium hydroxide (NaOH) is added to the buffer solution? The K₂ of formic acid is 1.8 x 104. (Two decimal places) Type your answer...

Like other people, I have been able to do more cooking and baking during COVID quarantine and remote teaching and learning. One of the things that I have been learning to make is Irish brown bread, a rather tasty version of a “soda bread.” The bread is called a soda bread because it has baking soda (sodium bicarbonate) in it. Sodium bicarbonate is the conjugate base of carbonic acid. What is the pH of a 0.350 M solution of sodium bicarbonate? (pKa of carbonic acid = 6.35)

explain why the ph doesnt change significantly when a small amount of an acid or a base is added to a solution that contains equal amounts of the base NH3 and a salt of its conjugate acid NH4CL

3. Sulfurous acid, H,SO, is a weak acid capable of producing two ions. A) What is the pH of a 0.45 M solution of H,SO,? B) What is the equilibrium concentration of the sulfide ion, so,, in this solution?

You have chosen Methylamine 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 0.48 M in this salt. The desired pH of the buffer should be equal to 9.75. To prepare the buffer, a total volume of 550 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 0.98 M. (Remember the lesson on dilution: C1V1=C2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (round off final answer to 1 decimal place)