Guided textbook solutions created by Chegg experts Learn from step-by-step solutions for over 34,000 ISBNs in Math Chemistry 112 Spring 2007 Prof. Metz Exam 3 Practice Questions 1 and 2 refer to a solution made by dissolving 0.020 mol of benzoic acid (HC7H5O2) and 0.010 moles of sodium benzoate (NaC7H5O2) in enough water to make A solution is prepared by dissolving 17.2 g of ethylene glycol (CHO) in 0.500 kg of water. Which silver salt will precipitate first? A solution is made by dissolving 26.7 g urea, a nonelectrolyte, in 301 g water. chemistry The following chemical reaction takes place in aqueous solution: SnSO4(aq)+2KOH(aq)->Sn(OH)2(s)+K2SO4(aq) Write the net ionic equation for this reaction. (The vapor pressure of pure water is 23.8 torr at 25 C and 71.9 torr at 45 C.) Calculate the vapor pressure of this solution at 25 C. chemistry What is the pH of this mixture of weak acids? Question: Calculate The Molar Solubility Of Ag2CrO4 (Ksp = 1.1 × 10-12) At 25 C In Various Aqueous Solutions. It is defined as the number of moles of solute dissolved in a liter of solution and formula is defined as (m/v) x (1 Include the balanced chemical equation. Since we know pH = -log[H⁺] You can calculate the amount dissolved per liter: x = 10^(-pH) = 10^-1.25 = 0.0562mol/L Multiply by the volume and The Ksp for AgCl is 1.8 x 10-10 and that for Ag2CrO4 is 1.2 x 10-12. Homework Statement I have to calculate the KSP of Ag2CRo4. a. CaCl2 Readily soluble, strong electrolyte b. 5. Learn vocabulary, terms, and more with flashcards, games, and other study tools. Calculate the M, m, %m,m and mole fraction. Calculate the solubility of Ag2CrO4 in grams per liter. At 25° C, the solubility of Ag2CrO4 in water is 7.8×10!5 M. a) Write a balance chemical reaction for the dissolving of Ag2CrO4 and calculate the solubility product constant, Ksp, for Ag2CrO4. Chemistry archive containing a full list of chemistry questions and answers from May 05 2012. See the answer The value of Ksp for silver chromate, Ag2CrO4, is 9.0×10−12. Assume that the density of the solution is 1.00 g/mol. A solution of 100.0 mL of 0.200 M KOH is But x M from the dissolving of Ag2SO4 is very small compared to the ion present in the solution, it can be neglected. The AgNO3 will settle to the bottom without dissolving. Calculate the mass percent, molarity, molality, and mole fraction of KCl. Ksp AgCl= 1.5 x 10^-10 Ksp AgBr= 5.0 x 10^-13 Ksp Ag2CrO4= 1.9 x 10^-12 b. Silver chromate, Ag2CrO4(s), dissolves in water to give Ag^+ and CrO4^2-. Some Ag2CrO4 will precipitate. This data gives a relationship between amount of solute and volume of solution: 5.67 g KCl / Solution: (x) (0.0500 L) = 20.0 g / 97.9937 g mol¯ 1 0.68 % 0.78 % 0.90 % 6.8 % 7.8 % 10 of 20 A solution is 0.010 M in both Cu 2+ and Cd 2+. 3 To determine the unknown concentration a standard concentration curve or calibration curve is constructed from a series of The solution was made by dissolving 4.550 g of Na2SO4 in water using 125.0 mL volumetric Chemistry What is the molarity of a solution made by dissolving 100.065 g of SnBr2 in water and diluting with water to 1.00 L A)Calculate The Solubility In 0.200 M AgNO3 B)Calculate The Solubility In 0.200 M Na2CrO4 So dissolving x moles of HI per liter leads to proton molarity molarity of: [H⁺] = x. Thus, as silver ions are slowly added to solution, AgCl precipitates first, removing the chloride ions from solution. What is the ionic concentrations of Ag+ and CrO4^-2 in a saturated solution of Ag2CrO4 at 25C? Ksp of Ag2CrO4 is 1.9x10^-12 mole^3/dm^9? A solution of AgNO3 (100% dissociated) is added to the above solution, drop by drop. Which silver salt will precipitate first? If Cl – + 2 Calculate the pH of the Chemistry … 10 atm 58 atm 14 atm 7.3 atm A solution is made by dissolving 55g of KCl in enough water to make 1.00 L of solution. b)Calculate the solubility of Ag2CrO4 in a solution … The final volume of the solution is 515 mL. Ksp = [Ag+]2[CrO42– ] 1 point for correct expression (b) Calculate the concentration, in mol L−1, of Ag+(aq) in a saturated solution of Ag2CrO4 at 25 (b) Calculate the concentration in mol L–1, of Ag+ in a saturated solution of Ag2CrO4 at Even if a substance isn't very soluble, if what does dissolve, dissociates completely, then it is strong. If the density of the solution is 1.15 g/mL, what is the mass percent NaOH in the solution? 2 4. Ag2CrO4 A saturated solutions of KCl in 100 grams of water is cooled form 90c to 60c. When Cl- is added to the solution, both AgCl (Ksp = 1.8 x 10-10) and PbCl2 (Ksp = 1.7 x 10-5) precipitate from the solution. Problem #13: What is the molarity of a solution made by dissolving 20.0 g of H 3 PO 4 in 50.0 mL of solution? The following question refers to a solution that contains 1.93 M hydrofluoric acid, HF (Ka = 7.2 × 10–4 ), and 3.00 M hydroponic acid, HCN (Ka = 6.2 × 10–10). A solution is prepared by dissolving 2.0 g NaOH (FW = 40.0 g/mol) to 255 mL of solution. Determine the concentration of a solution made by diluting 75ml of 5.0M NaOH with 200.0 ml of water. A solution is 0.15 M in both Pb 2+ and Ag +. The boiling point of pure acetone is said to be 55.95 C. A solution was made by dissolving 3.75g 3.when molten magnesium oxide was electrolyzed for a certain period, 150 mg of Mg was deposited on the 4.London dispersal 5. (a) Write the equilibrium-constant expression for the dissolving of Ag2CrO4(s). If both & and I are constant then absorbance is directly proportional to the concentration of the solution. Predict in what period on the periodic table will the first element with an electron occupying a g-sublevel first appear? Acetylsalicylic acid (aspirin, HC 9 H 7 O 4) is a weak acid with Ka = 2.75x10 –5 at 25 C. 3.00 g of sodium acetylsalicylate (NaC 9 H 7 O 4) is added to 200.0 mL of 0.100 M solution of this acid. Determine the concentration of stock solution used when 40.0 ml of it are needed to make 800.0 ml of 0.20 M HC2H3O2 . The term "strong" refers to a substance that dissociates completely. EXAMPLE: What is the molarity of a solution made by dissolving 5.67 g of potassium chloride in enough water to make 100.0 mL of solution? What concentration of Cl- is necessary d. The concentration of CrO42- will increase. 9. A solution contains 1.0 x 10-2 M Ag+ and 2.0 x 10-2 M Pb2+. Some Ag2CrO4 will precipitate. This problem has been solved! Point B represents a saturated solution of AgCl in pure water, in which the [Ag + ] and [Cl - … c. Nothing will happen. Explain N2(g and O2(g are both colourless, while NO2(g is dark brown.the colour of the mixture becomes darker or lighter as the temperature lowered? Chem help? Ksp = (2x)^2(0.43) = 1.2 x 10^-5 x^2 = 1.4 x 10^-5 = 14 x 10^-6 taking the square root of both sides Determine the amount concentration of potassium ions and dichromate ions in a solution made by dissolving 44.7 g of potassium dichromate to make a volume of 205 mL. Calculate The Solubility Of Ag2CrO4 In Grams Per Liter. In a saturated solution of Ag3PO4 at 25 C, the concentration of Ag+(aq) is 5.3 × 10–5 M. The equilibrium The equilibrium- constant expression for the dissolving of Ag 3 PO 4 ( s ) in water is shown below. Start studying General Chemistry II Module 8 Lecture. Calculate the Ksp for a 2.3x10^-3 M saturated solution of AgCl2? A solution is made by dissolving 13 g of sucrose, C12H22O11, in 117 g of water, producing a solution with a volume of 125 mL at 20 C. What is the expected osmotic pressure at 20 C? Ag2CrO4(s) 2 Ag+(aq) + CrO42–(aq) Ksp = 2.6 10–12 at 25˚C (a) Write the equilibrium constant expression for the dissolving of Ag2CrO4. Point A represents a solution at equilibrium that could be produced by dissolving two sources of the Ag + ion such as AgNO 3 and AgCl in water. 12. Here is the simple online molar concentration calculator to calculate the molarity substance which is expressed as mol/L. As can be inferred, Ag+ ions react with 57. A solution is made by combining 10.0 mL of 17.5 M acetic acid with 5.54 g of sodium acetate and diluting to a total volume of 1.50 L. Calculate the pH of the solution. Ksp of Ag2CrO4 is 1.9x10^-12 mole^3/dm^9? What percentage of Cd 2+ remains in the solution when 99.9% of the Cu 2+ has been precipitated as CuS by adding sulfide? 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