Your job is to determine the concentration of ammonia in a commercial window cleaner. In the titration of a 25.0 mL sample of the cleaner, the equivalence point is reached after 19.6  mL of 0.144 M  HCl has been added.   What is the initial concentration of ammonia in the solution?      M ammonia    What is the pH of the solution at the equivalence point?      = pH

The final volume of buffer solution must be 100.00 mL and the final concentration of the weak acid must be 0.100 M. Based on this information, what mass of solid conjugate base should the student weigh out to make the buffer solution with a pH of 3.50? mass= Based on this information, what volume of acid should the student measure to make the buffer solution? volume = g ml.

Given a 1.00 L solution that is 0.60 M HF and 1.00 M KF, calculate the pH after 0.090 mol NaOH is added, and calculate the pH after 0.18 mol HCl is added to the original solution. Ka = 7.2×10^-4 pH = when NaOH is added pH = when HCl is added

What is a description of the salt that is used in a buffer solution? from the conjugate base from a weak acid O from the conjugate base of a weak base from the conjugate acid of a weak acid O from the conjugate acid of a strong base

What will the pH of 1.50 L of pure water water be if 2.0 mL of 4.0 M HCl is added?  By how much has the pH changed?               What will the pH of the solution in part b be if 2.0 mL of  4.0 M HCl is added?  By how much has the pH changed?             c. What will the pH of the buffer in part c be if 2.0 mL of  4.0 M HCl is added?  By how much has the pH changed?

Write out a chemical equation. (The chemical equation, for example, is NaOH + HCl ® HOH + NaCl.) Explain what the equivalence point is, what the pH is at the equivalence point in this reaction and why the pH is what it is.

When a 21.3 mL sample of a 0.473 M aqueous hydrofluoric acid solution is titrated with a 0.339 M aqueous sodium hydroxide solution, what is the pH at the midpoint in the titration?pH =

A solution of the weak acid HA is prepared by dissolving 2.20 g of HA in 100.0 mL water. The solution is titrated, and the equivalence point is reached after 31.1 mL of 0.500 M NaOH is dispensed. Calculate the molar mass of HA. molar mass: g/mol At the equivalence point in this titration, how can the solution pH be described? acidic basic O neutral

In a titration with 25.00 mL of a 0.1300 M diprotic acid, 40.00 mL of NaOH is used to reach the equivalence point.  What is the concentration of the NaOH solution?

When a 16.9 mL sample of a 0.334 M aqueous hypochlorous acid solution is titrated with a 0.475 M aqueous sodium hydroxide solution, what is the pH at the midpoint in the titration? pH =