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- If 500mL of 0.10M Ca2+ is mixed with 500mL of 0.10M SO42-, what mass of calcium sulfate will precipitate? Ksp for CaSO4 is 2.40 • 10-5. express answer to 3 significant figures. And include units.If a student combines specific amount CaCl2. 9H2O and Na2CO3 and obtained a solid precipitate. The student dissolve 1.37 gram of CaCl2. 9H2O in 25.0 mL of water and 0.984 g of Na2CO3 in 25.0 mL of water. The student is then combining the two solutions and observed the formation of a solid precipitate. The student filter the solution and recovered the precipitate. The following data were obtained for the experiment. Initial Mass of CaCl2. 9H2O 1.37 g Initial Mass of Na2CO3 0.984 g % yield of this experiment 87.4% 1. What is the balanced equation for this experiment?If a student combines specific amount CaCl2. 9H2O and Na2CO3 and obtained a solid precipitate. The student dissolve 1.37 gram of CaCl2. 9H2O in 25.0 mL of water and 0.984 g of Na2CO3 in 25.0 mL of water. The student is then combining the two solutions and observed the formation of a solid precipitate. The student filter the solution and recovered the precipitate. The following data were obtained for the experiment. Initial Mass of CaCl2. 9H2O 1.37 g Initial Mass of Na2CO3 0.984 g % yield of this experiment 87.4% Question 1. Determine the amount of the solid in (grams) that the student recovered in this experiment. Question 2. How many grams from the excess reactant remains unreacted in this experiment?
- Solid ammonium chromate is slowly added to 75.0 mL of a calcium acetate solution until the concentration of chromate ion is 0.0154 M. The maximum amount of calcium ion remaining in solution is M. Please answer asap Thanks!A 50.00 mL volume of 0.0600M K2CrO4 is mixed with 50.00 mL 0.0800 M AgNO3. Calculate the concentration of Ag+, CrO42-, K+, and NO3- at equilibrium. The solubility product of Ag2CrO4(s) is 1.20 x 10-12. Please show workOne mixes aqueous NaCl with aqueous AgNO3. NaCl. AgNO3and NaNO3all have appreciable solubility in water. AgCl has a solubility product constant Ksp of 1.6 x 10-10. If one mixes the NaCl solution with the AgNO3solution, one would suspect: a) no precipitate will form b) AgCl precipitate will form c) NaNO3 precipitate will form d) both AgCl and NaNO3 precipitates will form
- Find calculated k value per trial: Average k value: The initial volume of syringe was 15ml and I converted everything to L because that is what my manual said to do. I am confused with my excel spreadsheet as well. Am I doing my calculations correctly?Complete the following: 1. Random error, also called _________arises from the effects of uncontrolled variables in the measurement. 2. The ____________,measures how closely the data are clustered about mean. 3. The chemical equilibrium in which all the reactants and products are in the same phase are called____________. 4. Reaction that go to completion and never proceed in the reverse direction are said to be_____________ 5. The equation for buffer is the__________equation. 6. A ___________solution is one that resists changes in pH when small quantities of an acid or an alkali added to it. 7. __________is the pH of the pure, neutral and polyprotic1. The Ksp of Ca3(PO4)2 is 1.3 × 10−26. Estimate the solubility of this salt in units of g. L−12. If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 2.1? Explain you answer in a short sentence. Please only answer 2nd Question
- Calcium carbonate (e.g. from limestone) is relatively insoluble in water, and the solubilitydecreases with rising temperature. This is why CaCO3 precipitates out as ‘scale’ in hot water more readily than cold water. At a temperature of 20oC, calcium carbonate pKs= 8.8; at 35oC, pKs= 9.25. If you had water that was at equilibrium with excess calcium carbonate at 20oC and then raised the temperature to 35oC, what is the mass of CaCO3 that will precipitate out per litre of water? Hint: the difference in solubility will drive the reaction back to solid. CaCO3(s)↔Ca2++CO2−__K2S(aq) + __H3PO4(aq) ® __K3PO4(aq) + __H2S(g) In a reaction mixture of 14.2 mL of 0.42 M K2S and 6.0 mL of 0.85 M H3PO4: 1. The theoretical yield of H2S from this reaction mixture, in mL at STP is _______ mLSTP 2. If 120 mL at STP of H2S was isolated, the percent reaction yield is ______Solid cobalt (II) acetate is slowly added to 125 mL of 0.0945 M ammonium chromate solution. What is the concentration of cobalt required to just initiate precipitation? The Ksp of CoCrO4 is 7.1 * 10 -4. Report answer in scientific notation to two sig figs.
