10.4 Calculate the mL of 0.100 M EDTA needed to titrate 100.0 mL of a 0.0100...
Calculate the concentration of an EDTA solution of which 24.22 mL were needed to titrate the Ca2+ ions present in a 50.00 mL solution containing 246.7 mg CaCO3. Express your answer in terms of (a) molar concentration of EDTA and (b) Ca titer (mg Ca per mL of EDTA)
13. If 20.54 mL of a 0.01011 M EDTA solution is needed to titrate the Ca and Mg* in a 40.00 mL water sample, what is the water hardness of the sample in ppm? a) 0.520 ppm b) 20.8 ppm c) 208 ppm d) 260 ppm 520 ppm
Calculate the change in pH when 3.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3 (aq) and 0.100 M in NH4CI(aq). Consult the table of ionization constants as needed ДрН Calculate the change in pH when 3.00 mL of 0.100 M N2OH is added to the original buffer solution. АрН -
Consider the titration of 30.0 mL of 0.0100 M CoSO4 with 0.0150 M EDTA in a solution buffered to pH 9.00. Calculate pCo2+ at 20.0 mL of EDTA added. Report the answer to three significant figures.
Calculate the pH of a buffer made from mixing 10.0 mL of 0.100 M NaC3H2O, and 10.0 mL of 0.100 M HC,H,O2 pH 4.76 Calculate the pH of the buffer when 5.00 mL of a 0.0100 M NaOH solution is added. pH Calculate the pH of the buffer when 5.00 mL of a 0.0100 M HCl solution is added.
100.0 mL of 0.100 M sodium sulfide is mixed with 100.0 mL of 0.100 M chromium (III) nitrate. Calculate the mass of solid that forms and the concentration of the remaining species in solution: assume complete precipitation.
Calculate the change in pH when 3.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH, (aq) and 0.100 M in NHCl(aq). Consult the table of ionization constants as needed. ApH = Calculate the change in pH when 3.00 mL of 0.100 M NaOH is added to the original buffer solution. ApH =
Calculate the change in pH when 7.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH, (aq) and 0.100 M in NH, Cl(aq). Consult the table of ionization constants as needed. ApH = Calculate the change in pH when 7.00 mL of 0.100 M NaOH is added to the original buffer solution. ApH =
Calculate the change in pH when 4.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH, (aq) and 0.100 M in NH Cl(aq). Consult the table of ionization constants as needed. ApH = Calculate the change in pH when 4.00 mL of 0.100 M NaOH is added to the original buffer solution. ApH =
The metal ion Mn+ was titrated with 0.0500 M EDTA. The initial solution contained 100.0 mL of 0.0500 M metal ion (Mn+) buffered at a pH of 9.00. a) Calculate the equivalence volume (Veq). b) What is the concentration of the free metal ion at volume V = Veq/2. c) If the conditional formation constant, K’f = 5.4 X 1010, calculate the concentration of free metal ion at volume V = Veq.