If the Ksp for Ag2CrO4 is 7.1 x 10-12, will precipitation occur when 10 mL of 1.0 x 10-4 M AgNO3 is mixed with 10 mL of 1.0 x 10-3 M K2CrO4?
If the Ksp for Ag2CrO4 is 7.1 x 10-12, will precipitation occur when 10 mL of...
Does any solid Ag2CrO4 form when 5.3 10-5 g of AgNO3 is dissolved in 15 mL of 4.9 10-3 M K2CrO4? Assume no volume change. What is the Qsp and the Ksp?
Does any solid Ag2CrO4 form when 8.0 10-4 g of AgNO3 is dissolved in 15 mL of 6.6 10-5 M K2CrO4? Assume no volume change. (NOTE: Only ONE submission is allowed for the first part of this question.) Yes, precipitate will form. No, precipitate will not form. Qsp? Ksp?
If the Ksp of silver chromate (Ag2CrO4) is 1.1 x 10-12 and the silver ion concentration in the solution is 0.0005 M, what is the chromate ion concentration? 1.0 x 10-4 M 4.4 x 10-6 M 5.0 x 10-7 M 1.0 x 10-6 M 6.5 x 10-5 M
a) Silver chromate, Ag2CrO4 is sparingly soluble in water with a Ksp 112 x 10-12. What is the molar solubility. S, of silver chromate in pure water? Consult Textbook Numerical Answer b) What is the molar solubility in a 130 M solution of K2CrO? Numerical Answer: c) What is the molar solubility in a 130 M solution of AgNO3? Numerical Answer
. Would precipitation occur when 500 mL of a 0.04M solution of AgNO3 is mixed with 500 mL of a 0.002M solution of NaCl? Justify your answer by showing your calculations.
1a) Silver chromate, Ag2CrO4, has a Ksp of 8.99 × 10–12. Calculate the solubility in mol/L of silver chromate. 1b) Calculate the molar solubility of AgCl (Ksp = 1.6 × 10–10) in 0.0034 M sodium chloride at 25°C. 1c) If 30 mL of 5.0 × 10–4M Ca(NO3)2 are added to 70 mL of 2.0 × 10–4M NaF, will a precipitate occur? (Ksp of CaF2 = 4.0 × 10–11)
1. Precipitation of Ionic Solids 1. 250.0 mL of 0.0062 M AgNO3 and 250.0 mL of 0.00014 M Na2CO3 are combined. Will a precipitate form? (Ksp of Ag2CO3 = 8.1 x 10-12) 2. Determine the minimum concentration of sodium bromide required to cause the precipitation of silver bromide from a 5.8 x 10-4M solution of AgNO3. (Ksp of AgBr = 5.0 x 10-13)
QUESTION 2 Kep(Ag2CrO4) = 9,0 x 10-12, Ksp(BaSO4) = 1.1 x 10-10, Ksp (AgSCN) - 1.2 x 10-12 What is the correct order of the solubility of the above ionic compounds? (from smallest to greatest) a. BaSO4 → AgSCN → Ag2C+04 b. AgSCN → Ag2CrO4 → BaSO4 c. AgSCN → BaSO4 → Ag2C104 d. No correct order is found. e. BaSO4 → Ag2Cr04 → AgSCN
1. If the standard solutions had unknowingly been made up tobe 0.0024 M AgNO3 and 0.0040 M K2CrO4, would this have affected your results? Why? 2. If your curvette had been dirty, how would this have affected the value of ksp? 3. Using your determined value of ksp, calculate how manymilligrams of Ag2CrO4 will desolve in 10.0 mL of H2O? 4. The experimental procedure for this experiment has you add 5mL of 0.004 M AgNO3 to 5mL of 0.0024 M...
Will AgIO3 precipitate when 20 mL of 0.010 M AgNO3 is mixed with 10mL of 0.015M NaIO3? (Ksp of AgIO3 is 3.1 x 10 ^ -8) a AgIO3 precipitates b no AqIO3 precipitates