1. A sample containing a mixture of CuCl2(s) and KCl(s) with a mole fraction of 6.90% KCI was dissolved in water. An excess of AgNO3(s) Was added to the mixture, resulting in all the chloride being precipitated as AgCl(s). The AgCl(s) was collected and dried, then weighed to have a mass of 4.20 g. Calculate the masses of KCl(s) and CuCl2(s) in the

1. A sample containing a mixture of CuCl2(s) and KCl(s) with a mole fraction of 6.90% KCI was dissolved in water. An excess of AgNO3(s) Was added to the mixture, resulting in all the chloride being precipitated as AgCl(s). The AgCl(s) was collected and dried, then weighed to have a mass of 4.20 g. Calculate the masses of KCl(s) and CuCl2(s) in the

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The molecular equation for the reaction that take place when two aqueous solutions are mixed is given below. Na2CO3(aq) + MgCl2(aq)→ MgCO:( )+ NaCl( ) a. Predict the physical status of the products, using the solubility rules chart, and indicate below. MgCO3: NaCl: b. Write the balanced molecular equation. c. Write the balanced total ionic equation d. Write the balanced net ionic equation
A 2.85 g sample of NaCl and CaCl2 was dissolved in water, and an excess of AgNO3 was added to precipitate all of the chloride ions.The AgCl was collected and dried, and weighed to give 7.20 g of AgCl. How much NaCl and CaCl2 was in the sample? i g NaCl g CaCl2
A 4.534 g sample of a solid mixture was analyzed for baum ion. First the rock was crushed in a mortar and pestle. 100% of the sample was transferred to a beaker, where it was dissolved in 150.0 mL of d.i. water. to give 152 mL of solution. The aqueous sample was then analyzed by adding a small excess of sulfuric acid. The resultant reaction produced a precipitate of barium sulfate, which was collected by filtration, rinsed, dried and weighed. If O.5376 g of barium sulfate was obtained, what was the mass percent of barium in the original sample? What was the molar concentration barium in the 152 mL of solution prior to adding sulfuric acid? Show work clearly; include a balanced net ionic chemical equation, units and sig. figs.
Barium can be analyzed by precipitating it as BaS04 and determining the mass of the precipitate. When a 0.269 g sample of a barium compound was treated with excess H2S04, 0.0891 g of BaS04 formed. What percentage of barium is in the compound?
Write a balanced equation for the double-replacement precipitation reaction described, using the smallest possible integer coefficients. A precipitate forms when aqueous solutions of manganese(II) sulfate and ammonium carbonate are combined. Do not include states such as (s) or (aq). It is not necessarry for you to indicate which of the products is the precipitate.
2. A supplement was tested for iron content in a laboratory. First, a random sample of 10 tablets weighing a total of 13.7421 g was turned into fine powder. A scoop of this powder weighing 2.7544 g was then dissolved and precipitated as Fe(OH)3 which was then rinsed and ignited to a constant weight as Fe₂O3 (159.69 g/mol). The recorded constant weight of Fe₂O3 is 0.2629 g. a. What is the %Fe (55.85 g/mol) content of the supplement? b. What is the iron content of the supplement reported as g FeSO4.7H₂O (277.908 g/mol) per tablet?
A 1.50 g sample of KCl is dissolved in 36.0 mL of water. The resulting solution is then added to 32.0 mL of a 0.470 M CaCl2 (aq) solution. Assuming that the volumes are additive, calculate the concentrations of each ion present in the final solution. Concentration of K* ions = M Concentration of Ca2+ ions = M Concentration of Cl ions = M
To determine the amount of iron in a dietary supplement, a random sample of 23 tablets weighing a total of 847 g was ground into a fine powder. A 0.5046 g sample of the powdered tablets was dissolved and treated to precipitate the iron as Fe(OH)3(106.95g/mol). The precipitate was collected, rinsed, and ignited to a constant weight as Fe2O3.(159.69g/mol) yielding 0.5445 grams. Report the iron content of the dietary supplement as g FeSO4.7H₂O (277.91g/mol) per tablet. Unit should not be written in the box.
Consider the neutralization reaction 2 HNO3(aq) + Ba(OH)2(aq). 2 H2O(l) + Ba(NO3)2(aq) A 0.105 L sample of an unknown HNO3 solution required 42.5 mL of 0.250 M Ba(OH)2 for complete neutralization. Wha the concentration of the HNO3 solution? concentration: .098
A 2.37 g sample of a mixture of FeCl2 and Fe(NO3)2 is treated with excess AgNO3(aq). The precipitate is filtered off, dried and weighed. The dried precipitate weighs 4.05 g. What is the percentage by mass of FeCl2 in the original mixture? Your answer must be accurate to two sig figs.
1. Observe the physical properties of sulfur and antimony at room temperature. Note their physical state, color and solubility in carbon disulfide. The solubility may be observed qualitatively by dissolving a pinch of the powdered samples in about 3 ml of carbon disulfide and stirring until the solid sample has dissolved. Record your observations in the table below. Solubility in CS, Classification of the sample (Element/Compound) Sample Physical Color State Sulfur Antimony a. Was the system formed by the addition of sulfur to CS,, homogeneous or heterogeneous? b. Could its composition be varied or not? c. Explain your answer in la. d. Was the system formed by the addition of antimony to CS, homogeneous or heterogeneous? e. Explain your answer in 1d.
Many chemical compounds contain impurities. Crude potassium carbonate (K2CO3) obtained from the chemical supplier is assayed for purity in the following way: 8.450 g of crude potassium carbonate is weighed out into a flask and dissolved in water. The final volume was completed to 0.500 L with distilled water. 20.00 mL sample is taken from this solution and placed in a flask. Potassium carbonate is then titrated to the equivalence point with 17.80 mL of 0.2050 M HCl solution. What is the percent purity of potassium carbonate in this sample? K2CO3 + HCl  KCl + H2O + CO2