The magnesium and calcium ions present in seawater have the following concentrations: [Mg2+] = 059 M and [Ca2+] = 0.011 M. The ions can be separated by precipitation with KOH. At what pH will the selective precipitation of Mg2+ ion be triggered? Ksp(Mg(OH)2 = 2.06 x 10-13        Ksp(Ca(OH)2 = 4.68 x 10-6

Magnesium sulfate, MgSO4, is added to 210. mL of 2.40 x 10-2 M sodium hydroxide, NaOH, until precipitate just forms. How many grams of magnesium sulfate were added? Assume that the volume of the solution is not changed significantly by the addition of magnesium sulfate. Kp (Mg(OH)2) = 1.8 x 10-11 8

A student prepares an FeSCN2+ experimental sample by mixing:4.0 mL of 0.0025 M Fe(NO 3) 32.0 mL of 0.0025 M KSCN8.0 mL of 0.10 M HNO 3Based on a standard curve, it was determined that the concentration of FeSCN 2+ present in thesample at equilibrium was 2.52 × 10 -5 M. Based on this data, calculate the equilibrium constant forthe reaction of Fe 3+ with SCN– .

Calcium sulfate is only sparingly soluble.   CaSO4(s) ⇌ Ca2+(aq) + SO42-(aq) For this type of dissolution reaction the equilibrium constant, also known as the solubility product, is denoted Ks.In the reaction above, Ks = 8.0 x 10-6.When an excess of the solid is dissolved in water what is the maximum concentration of Ca2+(aq) in mol L-1?

9:55 AM | 0.0KB/s Chegg Home Student question Expert Q&A My solutions Skip question Vo LTE 4G Start Solving JA In the determination of chloride by the Mob method, what will be the equiliblium concentration of silver ions in mgil, on the basis of the solubility - product principle, when the chloride concentation has been reduced to 0.2 ma? (b) If the concentration of chromate indicator used is 5X M, how much excess silver ion in mgiL must be present before the formation of a red precipitate will begi(a) In the defermination of chloride by the Mohr method, what will be the equilibrium concentration of silver ions in meL., an the basis of the solubility. pcoduct principle, when the chloride concencration has beea reduced to 0.2m? (b) If the concentration of chromate indicator ased is 5 × 10³ M, bow much excess silver ion in mel, must be present before the formatice of a red precipitate will begin? (b) If the concentration of chromate indicator used is 5 x 10-3 M, how much excess silver…

[References) In an experiment to determine solubility product, a student examined the solubility behavior of M(IO3)2. For two trials at 25 °C, he found the following ion concentrations for his equilibrium solutions: [103] Solution 1 3.74 x 103 3.3 x 10-3 Solution 2 1.48 x 10-2 2.06 x 10-3 Write the equilibrium reaction for the dissolution of M(IO3)2 and be sure that you include (s), (aq), etc.: Calculate the Ksp for each Solution and then report the average Ksp- Solution1 Ksp = Solution 2 Ksp = Average Ksp =

stion 5 Calculate the molar solubility of silver carbonate, Ag2CO3, in a solution containing 0.030 M sodium carbonate, Na2C03. Ksp of Ag2CO3 = 8.1 * 10-12 О 25× 10-3 м 8.2 * 10-6 M 9,7 * 10-9 M 84 * 10-10 M 1.5 * 10-8 M

The equilibrium constant is 4.5×10-32 for the reaction Ni(CN-(aq) +→ NP* (aq) + 4 CN¯ (aq) Calculate the equilibrium concentration, expressed in units of nM (nanomolar), of cyanide (CN") for a solution that initially only contains 0.25 M of Ni(CN)42- (aq). Enter your answer in deimal notation and provide 3 significant figures. For example, enter 0.2531 as 0.253

Ag2CO3(s)⇄2Ag+(aq)+CO32−(aq) The chemical equation above represents the equilibrium that exists in a saturated solution of Ag2CO3. If S represents the molar solubility of Ag2CO3, which of the following mathematical expressions shows how to calculate S based on Ksp? a.) S=The square root of Ksp b.) S= The square root of Ksp/2 c.) S= 3 times the square root of Ksp/2 d.) S= 3 times the square root of Ksp/4