2. Calculate the solubility of AgBr at: a) zero ionic strength and b) in a solution containing Ba(NO,). 0 02 M and M SO4, 0.01M. AgBr: K, = 5.2 x 10 dag= 2.5 A° a . =3 A°
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- Calculate the solubility at 25°C of AgBr in pure water and in 0.47M NaI . You'll probably find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits.Calculate the solubility at 25°C of AgBr in pure water and in 0.49M NaCN. You'll probably find some useful data in the ALEKS Data resource. ksp=5.35×10−13 Round your answer to 2 significant digits.Two hypothetical salts, LM2 and LQ, have the same molar solubility in H2O. If Ksp for LM2 is 3.20 × 10–5, what is the Ksp value for LQ?
- Two hypothetical salts, LM2 and LQ, have the same molar solubility in H2O. If Ksp for LM2 is 3.20 10–5, what is the Ksp value for LQ?A saturated solution of AgI contains 0.05 M KNO3. The Ksp for AgI is 8.3 x 10-17 . As a first approximation, assume that the ionic strength of this solution is dominated by 0.05 M KNO3 Calculate μ. Using the EDH, calculate γAg+ and γI-. Taking activities into account, calculate [Ag+] and [I-] in this solution. Was the approximation in Q20a valid? It not, how could you amend your ionic strength calculation?Calculate the molar solubility of Ag2S in a solution maintained at pH 11.00 and where the concentration of free ammonia is 0.100 M. Ag2S: pKsp = 48.70H2S: Ka1 = 1.0 x 10-7 ; Ka2 = 1.2 x 10-15[Ag(NH3)2]+: Kf1 = 2.04 x 103 ; Kf2 = 8.13 x 103
- Calculate the molar solubility (in mol/L) of Ag2S(s) at 25 °C in a solution of 0.30 M Na2S(aq). Ksp for Ag2S at 25 °C is 6.0x10–50The reaction A(g) + B(g) ↔ C(g) + D(g) has ΔGrxn° = -28.62 kJ mol-1 and Kp = 0.63 at 980 °C. A rigid cylinder at that temperature contains 1.2 atm of A, 0.20 atm of B, 0.30 atm of C, and 0.27 atm of D. What is the reaction Gibbs energy?Calculate the solubility at 25C of AgCl in pure water and in a 0.0170 M AgNO3 solution.
- calculate the molar solubility of AgBr in 3.1×10−2 M AgNO3 solution. Ksp = 5.0x10-13 for AgBrCalculate the solubility of CaF2 (aq) in a solution, that is 0.015 molar in MgSO4 (aq). Compare your result to the one you obtain by using concentration instead of activities. Take the solubility product as 3.9 × 10 ^-11When silver chromate, Ag2CrO4, dissolves in otherwise pure water, what is the relation between [Ag+] and [CrO42-]? The solubility product of Ag2CrO4 is 1.9x10-12. Show that its solubility in pure water is 0.78x10-4 M.