Question

In: Chemistry

500ml of each of 0.200 M NaF and 0.050 M CaCl2 are mixed. Calculate the concentration...

500ml of each of 0.200 M NaF and 0.050 M CaCl2 are mixed. Calculate the concentration of Ca^2+ remaining in solution after the precipitation of CaF2 is complete.

Ksp of CaF2 = 3.4x10^-11

A)0.05M

B)0.025M

C)3.4x10^-9M

D)1.7x10^-10M

E)1.4x10^-8M

Solutions

Expert Solution


Related Solutions

50.0 ml of 0.200 M AgNO3 is mixed with 50.0 ml of 0.050 M NaCl. Calculate...
50.0 ml of 0.200 M AgNO3 is mixed with 50.0 ml of 0.050 M NaCl. Calculate the concentration of Ag + and Cl- in the resulting solution, assuming the volumes are additive. Ksp(AgCl) = 1.82*10-10
Calculate the concentration of Ca2+ in a saturated solution of CaSO4 that contains 0.1 M CaCl2....
Calculate the concentration of Ca2+ in a saturated solution of CaSO4 that contains 0.1 M CaCl2. Ksp= 2.5*10-5 for CaSO4.
Calculate the hydronium ion concentration and pH for a 0.050 M solution of sodium formate, NaHCO2....
Calculate the hydronium ion concentration and pH for a 0.050 M solution of sodium formate, NaHCO2. Kb for reaction of HCO2- ion with water is 5.6 × 10-11. [H3O+] =_____ M pH =______
25.0 mL of 0.200 M solution of HBr are mixed with 25.0 mL of 0.200 M...
25.0 mL of 0.200 M solution of HBr are mixed with 25.0 mL of 0.200 M solution of NaOH in a constant pressure calorimeter. The temperature increases from 23.00 °C to 24.37 °C. Assume that the specific heat of the solution is the same as that of pure water (4.18 J/(g•°C)) and that the density is the same as pure water (1.00 g/mL). Calculate ΔH per mole of reaction for the below chemical reaction. HBr (aq) + NaOH (aq) →...
Consider the titration of 0.050 M HCl with 0.050 M NaOH. Calculate the pH: (a) of...
Consider the titration of 0.050 M HCl with 0.050 M NaOH. Calculate the pH: (a) of the pure HCl solution; (b) of 25.00 mL acid plus 12.50 mL base; (c) at the quivalence point; and (d) of 25.00 mL acid and 37.50 mL base.
Calculate the pH at the equivalence point in titrating 0.050 M solutions of each of the...
Calculate the pH at the equivalence point in titrating 0.050 M solutions of each of the following with 0.043 M NaOH. (a) hydrochloric acid (HCl) pH =   (b) ascorbic acid (HC6H7O6), Ka = 8e-05 pH =   (c) hypoiodous acid (HIO), Ka = 2.3e-11 pH =  
Calculate the pH for each case in the titration of 50.0 mL of 0.200 M HClO(aq)0.200...
Calculate the pH for each case in the titration of 50.0 mL of 0.200 M HClO(aq)0.200 M HClO(aq) with 0.200 M KOH(aq).0.200 M KOH(aq). Use the ionization constant for HClO. What is the pH before addition of any KOH? pH= What is the pH after addition of 25.0 mL KOH? pH= What is the pH after addition of 35.0 mL KOH? pH= What is the pH after addition of 50.0 mL KOH? pH= What is the pH after addition of...
Calculate the pH for each case in the titration of 50.0 mL of 0.200 M HClO(aq)0.200...
Calculate the pH for each case in the titration of 50.0 mL of 0.200 M HClO(aq)0.200 M HClO(aq) with 0.200 M KOH(aq).0.200 M KOH(aq). Use the ionization constant for HClO.HClO. What is the pH before addition of any KOH?KOH? pH=pH= What is the pH after addition of 25.0 mL KOH?25.0 mL KOH? pH=pH= What is the pH after addition of 35.0 mL KOH?35.0 mL KOH? pH=pH= What is the pH after addition of 50.0 mL KOH?50.0 mL KOH? pH=pH= What...
Calculate the pH of a buffer that is 0.10 M in KH2PO4 and 0.050 M in...
Calculate the pH of a buffer that is 0.10 M in KH2PO4 and 0.050 M in Na2HPO4. What is the pH after adding 5.0 mL of 0.20 M HCl to 0.10 L of this buffer. The Ka value for H2PO4– is 6.32 × 10–8 or a pKa of 7.199
A volume of 84 mL of 0.060 M NaF is mixed with 28 mL of .15...
A volume of 84 mL of 0.060 M NaF is mixed with 28 mL of .15 M Sr(NO3)2. Calculate the concentrations of the following ions in the final solution (Ksp for SrF2 is 2.0x10^-10)
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT