QUES A certain compound was known to contain calcium and chlorine. A sample that weighed 2.78g was dissolved in water, and excess sodium oxalate solution was added to precipitate all the calcium as calcium oxalate, CaC204. The equation for this reaction was: Ca* (aq)+ C,0, (ag)→ CaC,0,(s) The precipitate was then collected by filtration and heated strongly so that calcium oxide, CaO, formed. The calcium oxide was found to have a mass of 1.40 g. What was the empirical formula of the compound?

QUES A certain compound was known to contain calcium and chlorine. A sample that weighed 2.78g was dissolved in water, and excess sodium oxalate solution was added to precipitate all the calcium as calcium oxalate, CaC204. The equation for this reaction was: Ca* (aq)+ C,0, (ag)→ CaC,0,(s) The precipitate was then collected by filtration and heated strongly so that calcium oxide, CaO, formed. The calcium oxide was found to have a mass of 1.40 g. What was the empirical formula of the compound?

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...

See similar textbooks

Similar questions

An iron ore sample weighing 0.9174 g is dissolved in HCl(aq), and the iron is obtained as Fe2+(aq). This solution is then titrated with 34.62 mL of 5.016×10−2 M K2Cr2O7(aq)6Fe2+ + 14H+ + Cr2O2−7 → 6Fe3+ + 2Cr3+ + 7H2O What is the mass percent Fe in the ore sample?
You are asked to determine the percentage of the components of a mixture containing sodium iodide, NaI, magnesium hydroxide, Mg(OH)2, and barium sulfate, BaSO4. The total mass of your mixture sample is 4.82g. First you extracted the NaI from the mixture with water and filtered insoluble Mg(OH)2 and BaSO4 from the solution, containing the NaI. After evaporating and drying the filtrate, you find that you have recovered 0.95g of NaI. When you react the insoluble residue of Mg(OH)2 and BaSO4 with 3M HCl, the Mg(OH)2 dissolves. After decanting the supernatant liquid containing aqueous MgCl2 from the insoluble BaSO4 and drying the solid, you recover 2.04g of BaSO4. Finally you add 3M KOH solution to the aqueous solution to precipitate the Mg(OH)2. After filtering thesolution and drying the precipitate, you recovered 1.21g of Mg(OH)2. Calculate the percent Mg(OH)2 in the original sample mixture.
You are asked to determine the percentage of the components of a mixture containing sodium iodide, NaI, magnesium hydroxide, Mg(OH)2, and barium sulfate, BaSO4. The total mass of your mixture sample is 4.82g. First you extracted the NaI from the mixture with water and filtered insoluble Mg(OH)2 and BaSO4 from the solution, containing the NaI. After evaporating and drying the filtrate, you find that you have recovered 0.95g of NaI. When you react the insoluble residue of Mg(OH)2 and BaSO4 with 3M HCl, the Mg(OH)2 dissolves. After decanting the supernatant liquid containing aqueous MgCl2 from the insoluble BaSO4 and drying the solid, you recover 2.04g of BaSO4. Finally you add 3M KOH solution to the aqueous solution to precipitate the Mg(OH)2. After filtering thesolution and drying the precipitate, you recovered 1.21g of Mg(OH)2.
A chemist performs a gravimetric analysis. The chemist combines 1.00 L of 2.00 M AGNO, (ag) with 1.00 L of 4.00 M NaCl (aq) in an Erlenmeyer flask. Both the AGNO, (aq) solution and the NaCl(ag) solution are colorless. After the mixture has been stirred, a cloudy white substance is observed at the bottom of the flask. Which of the following is the complete ionic equation for the reaction that occurs in the beaker? A Ag+ (ag) + Cl- (aq) → AgCl (s) B Na (aq) + NO3 (aq) → NANO3 (s) Ag (aq) + NO, (aq) + Na (aq) + Cl-(aq) → AgCl(s) + Na* (aq) + NO, (aq) NaCl(aq) + AGNO, (aq) Ag (s) + NANO, (aq)
When the following solutions are mixed together, what precipitate (if any) will form? Note: Leave the answer blank if no precipitate will form. (Express your answer as a chemical formula.) Formula of precipitate Na,SO4(ag) + Pb(NO3)2(aq) – (s) KCI(ag) + NANO3(aq) → |(s) KOH(aq) + Mn(NO3)2(aq) – |(s)
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.
Lead ions can be precipitated from solution with KC1 according to the following reaction: Pb²+ (aq) + 2 KCl(aq) → PbCl₂(s) + 2 K+ (aq) When 28.8 g KCl is added to a solution containing 25.5 g Pb²+, a PbCl₂ precipitate forms. The precipitate is filtered and dried and found to have a mass of 29.6 g. Part A Determine the limiting reactant. KCI Pb²+ Submit Part B m = Determine the theoretical yield of PbCl₂. Submit Part C Request Answer ΨΕ ΑΣΦ Submit Request Answer Determine the percent yield for the reaction. ΨΕ ΑΣΦ Request Answer BE ? ? % g
Solution A is 0.2400 M Ca(NO3)2(aq).Solution A is diluted by a factor of 3 to form Solution B.As2O3(s) reacts with NO3–(aq) to produce NO(g) and H3AsO4(aq)When As2O3(s) was added to 27.50 mL of Solution B, 1.710 × 1021 molecules of NO(g) wereobtained from the reaction in 88.75% yield.(a) If As2O3(s) was the limiting reactant, calculate the mass of As2O3(s) which reactedwith NO3–(aq).(b) Determine the number of moles of NO3– in the 27.50 mL of Solution B which remained unreacted at the end of the reaction
A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 17.07 g PbCl2(s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq) solution.
McQuarrie · Rock Gallogly A 0.3146 g sample of a míxture of NaCI(s) and KBr(s) was dissolved in water. The resulting solution required 37.40 ml. of 0.08765 M AGNO, (aq) to precipitate the CI (aq) and Br (aq) as AgCI(s) and AgBr(s). Calculate the mass percentage of NaCI(s) in the mixture. mass percentage: % NaCI
The zinc content of a 1.55 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc. The excess HCl is then neutralized with with NaOH. The reaction of HClHCl with Zn is shown. Zn(s)+2HCl(aq)⟶ZnCl2⁢(aq)+H2⁡(g) The ore was dissolved in 150 mL of 0.600 M HCl and the resulting solution was diluted to a total volume of 300 mL. A 20.0 mL aliquot of the final solution required 8.92 mL of 0.548 NaOH to neutralize the excess HCl. What is the mass percentage (%w/w) of Zn in the ore sample?
You are asked to determine the percentage of the components of a mixture containing sodium iodide, NaI, magnesium hydroxide, Mg(OH)2, and barium sulfate, BaSO4. The total mass of your mixture sample is 4.82g. First you extracted the NaI from the mixture with water and filtered insoluble Mg(OH)2 and BaSO4 from the solution, containing the NaI. After evaporating and drying the filtrate, you find that you have recovered 0.95g of NaI. When you react the insoluble residue of Mg(OH)2 and BaSO4 with 3M HCl, the Mg(OH)2 dissolves. After decanting the supernatant liquid containing aqueous MgCl2 from the insoluble BaSO4 and drying the solid, you recover 2.04g of BaSO4. Finally you add 3M KOH solution to the aqueous solution to precipitate the Mg(OH)2. After filtering thesolution and drying the precipitate, you recovered 1.21g of Mg(OH)2. Calculate the total percent recovery based on the combined masses that were recovered.