megan

A sample of 0.214 g of an unknown monoprotic weak acid was dissolved in 25 ml of water and titrated with 0.095M NaOH. The acid required 15.5 ml of NaOH to reached the equivalence point. What is the molar mass of the unknown acid?

A buffer is made by adding 10.75 g of acetic acid (Ka=1.8x10^-5) and 10.75 g of sodium acetate in enough water to make 100 ml of solution. Calculate the pH of this buffer after 25 ml of 1M NaOH has been added. Please show calculations! Thank you:)

m(NH3)/m(NH4Cl)

A)titration will require more moles of acid than base to reach the equivalence point.

B)pH will be greater than 7 at the equivalence point.

C)pH will be less than 7 at the equivalence point.

D)titration will require more moles of the base than acid to reach the equivalence point.

E)pH will be 7 at the equivalence point.

What is the pH of a solution made by mixing 5.00 mL of 0.10 M acetic acid with 5.00 mL of 0.10 M KOH? Assume that the volumes of the solutions are additive. K a = 1.8

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10-5 for CH3CO2H.

To form the chloratw ion and copper (ii) ion in an aqueous solution. Use the smallest while # coefficients possible.