a.Sr(NO3)2(aq) + 2KF(aq) -------> SrF2(s) + 2KNO3(aq)
b. Sr^2+(aq) + 2(NO3)^-(aq) + 2K^+(aq) + 2F^-(aq) -------> SrF2(s) + 2K^+(aq) + 2NO3^-(aq)
Removal of spectator ions to get net ionic equation
Sr^2+(aq) + 2F^-(aq) -------> SrF2(s)
c. SrF2(s) ----------> Sr^2+ (aq) + 2F^- (aq)
KSp = [Sr^2+][F^-]^2
Qsp = [Sr^2+][F^-]^2
d.
Qsp = [Sr^2+][F^-]^2
= 2.1*10^-4 *(0.0044)
= 9.24*10^-7
Ksp = 7.9*10^-10
Qsp > KSp
e.Qsp > KSp precipitate will form
3. A solution containing potassium bromide is mixed with one containing strontium nitrate to form a...
A solution containing potassium bromide is mixed with one containing lead acetate to form a solution that is 0.013 M in KBr and 0.0035 M in Pb(C2H3O2)2. Will a precipitate form in the mixed solution? If so, identify the precipitate. Express your answer as a chemical formula. Enter noreaction if no precipitate is formed.
A solution containing sodium fluoride is mixed with one containing calcium nitrate to form a solution that is 0.015 M in NaF and 0.010 M in Ca(NO3)2 Will a precipitate form in the mixed solution? If so, identify the precipitate. Express your answer as a chemical formula. Enter noreaction if no precipitate is formed. Submit Request Answer
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At 25 0C the solubility product constant, Ksp, for strontium sulfate, SrSO4, is 7.6 x 10-7. The solubility product constant for strontium fluoride, SrF2, is 7.9 x 10-10. (a) What is the molar solubility of SrSO4 in pure water at 25 0C? (b) What is the molar solubility of SrF2 in pure water at 25 0C? (c) An aqueous solution of Sr(NO3)2 is added slowly to 1.0 litre of a well-stirred solution containing 0.020 mole F- and 0.10 mole SO42-...
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if 125 mL of a solution containing 0.0400 M of Pb(NO3)2 (aq) is mixed with 75.0 mL of a solution containing 0.0200 of NaCl(aq), will there be a precipitate? PbCl3 has a Ksp value of 1.6 x 10^-5. Assume volumes are additive when mixed
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