Answer all parts of the following: a. When solutions of Pb2+ and CrO42− are mixed the...
Answer all parts of the following:
a. When solutions of Pb2+ and CrO42− are mixed the precipitate PbCrO4 is produced. What volume of 0.2150 M CrO42− removes all lead from 50.00 mL of a 0.3345 M Pb2+ solution?
b. What volume of a 50.0% by mass NaOH solution must be diluted to prepare a 0.4500 M NaOH solution with a volume of 500 mL? The density of 50% NaOH solution is 1.515 g/mL at 25°C.
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Answer all parts of the following:
a. When solutions of Pb2+ and CrO42− are mixed the...
Questions 1 & 2 refer to the solubility of lead chromate, PbCrO4: PbCrO4(s) = Pb2+ (aq) + CrO42-(aq) 1. The Ks for...
Questions 1 & 2 refer to the solubility of lead chromate, PbCrO4: PbCrO4(s) = Pb2+ (aq) + CrO42-(aq) 1. The Ks for PbCrO4 is 2.0 x 10-16 at 25 °C. What is the solubility of PbCrO4 in mol L-?? a) 1.4 x 10-8 b) 2.8 x 10-8 c) 2.0 10-16 d) 7.1 x 10 e) 5.0 x 1015 2. If 5.0 mL of 1.0 x 10-'M Pb(NO3)2 is added to 5.0 mL of a solution of 1.0 x 10-0MK2Cr04, which...
Be sure to answer all parts. One way to remove lead ion from water is to...
Be sure to answer all parts. One way to remove lead ion from water is to add a source of iodide ion so that lead iodide will precipitate out of solution: Pb2+(aq) + 2I−(aq) → PbI2(s) (a) What volume of a 1.0 M KI solution must be added to 210.0 mL of a solution that is 0.13 M in Pb2+ion to precipitate all the lead ion? (b) What mass of PbI2 should precipitate?
Be sure to answer all parts. You are given solutions of HCl and NaOH and must...
Be sure to answer all parts. You are given solutions of HCl and NaOH and must determine their concentrations. You use 82.6 mL of NaOH to titrate 100. mL of HCl and 12.4 mL of NaOH to titrate 50.0 mL of 0.0782 M H2SO4. Find the unknown concentrations. ____ M NaOH ____ M HCl Be sure to answer all parts. You are given solutions of HCl and NaOH and must determine their concentrations. You use 82.6 mL of NaOH to...
Please answer all parts of this question. Part A Constants 1 Periodis Table Before mixing, how...
Please answer all parts of this question.
Part A Constants 1 Periodis Table Before mixing, how many grams of Cu are present in the solution of CusO, Express your answer using three significant figures. Consider two solutions, the first being 50.0 mL of 1.00 M CuSO4 and the second 50.0 mL of 2.00 M KOH. When the two solutions are mixed in a constant-pressure calorimeter, a precipitate forms and the temperature of the mixture rises from 21.5°C to 27.70 C....
Part A When 75.5 mL of a 0.100 M lead (II) nitrate solution is mixed with...
Part A When 75.5 mL of a 0.100 M lead (II) nitrate solution is mixed with 104.5 mL of a 0.185 M potassium iodide solution, a yellow-orange precipitate of lead (II) iodide is formed What mass (in grams) of lead (II) iodide is formed, assuming the reaction goes to completion? Submit My Answers Give Up Part B What is the molarity of Pb2+ in the resulting solution? Pb2+ molarity = Submit My Answers Give Up Part C What is the...
Select all of the following solutions that would form a buffer when they were mixed. A...
Select all of the following solutions that would form a buffer when they were mixed. A solution that is formed when 0.82 moles of NH3 is mixed with 0.24 moles of HBr. Assume the final volume is 1.0 L. A solution that is formed when 0.52 moles of NaNO2 is mixed with 0.24 moles of HCl. Assume the final volume is 1.0 L. A solution that is formed when 0.23 moles of CH3CH2COOH is mixed with 0.49 moles of NaOH....
This question has multiple parts. Work all the parts to get the most points. When the following solutions are mixed...
This question has multiple parts. Work all the parts to get the most points. When the following solutions are mixed together, what precipitate (if any) will form? (Express your answer as a chemical formula. Enter none if no precipitate forms. Omit states of matter.) a K S(aq) + Ni(NO3)2(aq) Precipitate: b Hg, (NO3)2 (aq) + CuSO4 (aq) Precipitate: C Al(NO3)3(aq) + Ba(OH)2(aq) Precipitate: d K,Cos (aq) + Mg12(aq) Precipitate
When 25.0 mL of 0.700 mol/L NaOH was mixed in a calorimeter with 25.0 mL of...
When 25.0 mL of 0.700 mol/L NaOH was mixed in a calorimeter with 25.0 mL of 0.700 mol/L HCl, both initially at 20.0 °C, the temperature increased to 22.1 °C. The heat capacity of the calorimeter is 279 J/°C. Since the solutions are mostly water, the solutions are assumed to have a density of 1.0 g/mL and a specific heat of 4.18 J/g°C. What is the mass of the solution? Select one: a. No enough information b. 50.0 g c. 50.0 kg d. 25.0...
When 50.0 mL of 1.00 M HCl and 50.0 mL of 1.00 M NaOH are mixed...
When 50.0 mL of 1.00 M HCl and 50.0 mL of 1.00 M NaOH are mixed in a constant-pressure calorimeter, the temperature of the solution increases from 21.0°C to 27.5°C. Calculate the enthalpy change of the reaction per mole of HCl assuming the solution has a total volume of 100.0 mL and a density of 1.000 g/mL. The specific heat of water is 4.184 J/q°C Asoln = 2720
Be sure to answer all parts. A student mixes 50.0 mL of 1.00 M Ba(OH)2 with...
Be sure to answer all parts. A student mixes 50.0 mL of 1.00 M Ba(OH)2 with 76.2 mL of 0.450 M H2SO4. Calculate the mass of BaSO4 formed. g Calculate the pH of the mixed solution.=
Questions 1 & 2 refer to the solubility of lead chromate, PbCrO4: PbCrO4(s) = Pb2+ (aq) + CrO42-(aq) 1. The Ks for PbCrO4 is 2.0 x 10-16 at 25 °C. What is the solubility of PbCrO4 in mol L-?? a) 1.4 x 10-8 b) 2.8 x 10-8 c) 2.0 10-16 d) 7.1 x 10 e) 5.0 x 1015 2. If 5.0 mL of 1.0 x 10-'M Pb(NO3)2 is added to 5.0 mL of a solution of 1.0 x 10-0MK2Cr04, which...
Please answer all parts of this question.
Part A Constants 1 Periodis Table Before mixing, how many grams of Cu are present in the solution of CusO, Express your answer using three significant figures. Consider two solutions, the first being 50.0 mL of 1.00 M CuSO4 and the second 50.0 mL of 2.00 M KOH. When the two solutions are mixed in a constant-pressure calorimeter, a precipitate forms and the temperature of the mixture rises from 21.5°C to 27.70 C....
Part A When 75.5 mL of a 0.100 M lead (II) nitrate solution is mixed with 104.5 mL of a 0.185 M potassium iodide solution, a yellow-orange precipitate of lead (II) iodide is formed What mass (in grams) of lead (II) iodide is formed, assuming the reaction goes to completion? Submit My Answers Give Up Part B What is the molarity of Pb2+ in the resulting solution? Pb2+ molarity = Submit My Answers Give Up Part C What is the...
This question has multiple parts. Work all the parts to get the most points. When the following solutions are mixed together, what precipitate (if any) will form? (Express your answer as a chemical formula. Enter none if no precipitate forms. Omit states of matter.) a K S(aq) + Ni(NO3)2(aq) Precipitate: b Hg, (NO3)2 (aq) + CuSO4 (aq) Precipitate: C Al(NO3)3(aq) + Ba(OH)2(aq) Precipitate: d K,Cos (aq) + Mg12(aq) Precipitate
When 50.0 mL of 1.00 M HCl and 50.0 mL of 1.00 M NaOH are mixed in a constant-pressure calorimeter, the temperature of the solution increases from 21.0°C to 27.5°C. Calculate the enthalpy change of the reaction per mole of HCl assuming the solution has a total volume of 100.0 mL and a density of 1.000 g/mL. The specific heat of water is 4.184 J/q°C Asoln = 2720
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