Chemistry Homework Questions

Calculate the pH after 0.017 mole of HCl is added to 1.00 L of each of the four solutions. (Assume that all solutions are at 25°C.)

(a)    0.133 M acetic acid (HC2H3O2Ka = 1.8  10−5)

(b)    0.133 M sodium acetate (NaC2H3O2)

(c)    pure H2O

(d)    0.133 M HC2H3O2 and 0.133 M NaC2H3O2


Consider a solution that contains both C6H5NH2 and C6H5NH3+. Calculate the ratio [C6H5NH2]/[C6H5NH3+] if the solution has the following pH values. (Assume that the solution is at 25°C.)

(a)    pH = 5.16

(b)    pH = 5.53

(c)    pH = 4.74

(d)    pH = 4.93


Consider the titration of 41.5 mL of 0.198 M HCl with 0.124 M NaOH. Calculate the pH of the resulting solution after the following volumes of NaOH have been added. (Assume that all solutions are at 25°C.)

(a)    0.0 mL

(b)    10.0 mL

(c)    40.0 mL

(d)    80.0 mL

(e)    100.0 mL

Consider the titration of 100.0 mL of 0.240 M benzoic acid (Ka = 6.4  10−5) with 0.120 M KOH. Calculate the pH of the resulting solution after each of the following volumes of KOH has been added. (Assume that all solutions are at 25°C.)

(a)    0.0 mL

(b)    50.0 mL

(c)    100.0 mL

(d)    150.0 mL

(e)    200.0 mL

(f)    250.0 mL


Calculate the pH at the halfway point and at the equivalence point for each of the following titrations. (Assume that the temperature is 25°C.)

(a)    101.1 mL of 0.17 M HF (Ka= 7.2  10−4) titrated with 0.17 M KOH

halfway point
equivalence point

(b)    100.7 mL of 0.15 M C2H5NH2 (Kb = 5.6  10−4) titrated with 0.30 M HNO3

halfway point
equivalence point

(c)    100.9 mL of 0.51 M HCl titrated with 0.26 M KOH

halfway point
equivalence point








Calculate the solubility of each of the following compounds in moles per liter. Ignore any acid-base properties.

(a)    Ca3(PO4)2Ksp = 1.3  10−32

(b)    MgF2Ksp = 6.4  10−9

(c)    AgBr, Ksp = 5.0  10−13


The Ksp for silver chromate (Ag2CrO4) is 9.0  10−12. Calculate the solubility of silver chromate in each of the following.

(a)    water

(b)    0.15 M AgNO3

(c)    0.34 M Na2CrO4



Use the following data to calculate the Ksp value for each solid.

(a) The solubility of MnCO3 is 1.1  10−3 g/L.

(b) The solubility of Al(OH)3 is 5.5  10−9 mol/L.



The concentration of Ba2+ in a solution saturated with BaF2(s) is 1.82  10−2 M. Calculate Ksp for BaF2.






Calculate the solubility (in mol/L) of Co(OH)3 (Ksp = 3  10−43) in each of the following. (Assume that all solutions are at 25°C.)

(a) water (assume pH is 7.0 and constant)

(b) a solution buffered at pH = 5.5

(c) a solution buffered at pH = 10.9






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