Consider the following chemical reaction. 3 Zn(C:H:O2)>(aq) + 2 NasPO:(aq) –→ 6 NaCaHsOz(aq) + Zn:(PO:):(s) a) If sodium phosphate is in excess in the following balanced chemical equation, what compound is the limiting reactant? b) A chemist makes a solution of zinc acetate by dissolving 20.5 g Zn(C2HSO2)2 in 105 mL H2O. What is the concentration of this zinc acetate solution? c) How many moles of aqueous zinc acetate will react with excess aqueous sodium phosphate to precipitate one mole of solid zinc phosphate? d) The chemical formula of zinc phosphate is Zn:(PO+).. What is the formula weight of zinc phosphate? Provide an answer to two decimal places. e) Calculate the mass in grams Zn:(PO.)2 that can be precipitated from 0.105 L of a 1.06 M Zn(C2H:O2)2 Solution by the reaction with excess aqueous sodium phosphate (Na:PO4) according to the following balanced chemical equation: 3 Zn(CzH:O2):(aq) + 2 Na:PO:(aq) → 6 NaC:H:O:(aq) + Zn:(PO+):(s) f) In the reaction of 20.5 grams of Zn(C:H:O2). with excess NasPO4, would you expect the total mass of Zns(PO.)2 precipitated to be greater than, less than, or equal to the mass of the zinc acetate?

Consider the following chemical reaction. 3 Zn(C:H:O2)>(aq) + 2 NasPO:(aq) –→ 6 NaCaHsOz(aq) + Zn:(PO:):(s) a) If sodium phosphate is in excess in the following balanced chemical equation, what compound is the limiting reactant? b) A chemist makes a solution of zinc acetate by dissolving 20.5 g Zn(C2HSO2)2 in 105 mL H2O. What is the concentration of this zinc acetate solution? c) How many moles of aqueous zinc acetate will react with excess aqueous sodium phosphate to precipitate one mole of solid zinc phosphate? d) The chemical formula of zinc phosphate is Zn:(PO+).. What is the formula weight of zinc phosphate? Provide an answer to two decimal places. e) Calculate the mass in grams Zn:(PO.)2 that can be precipitated from 0.105 L of a 1.06 M Zn(C2H:O2)2 Solution by the reaction with excess aqueous sodium phosphate (Na:PO4) according to the following balanced chemical equation: 3 Zn(CzH:O2):(aq) + 2 Na:PO:(aq) → 6 NaC:H:O:(aq) + Zn:(PO+):(s) f) In the reaction of 20.5 grams of Zn(C:H:O2). with excess NasPO4, would you expect the total mass of Zns(PO.)2 precipitated to be greater than, less than, or equal to the mass of the zinc acetate?

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

A student prepared a Kool-Aid solution from 1.3151 g of Kool-Aid in a 100mL volumetric flask. In an experiment a student used 20.15 mL of 0.0200 M NaOH to titrate a 10.00 mL aliquot of this Kool-Aid solution. To calculate the mass % of citric acid in the aliquot we use: mass % of Kool-Aid = (mass of citric o cidla)V (nmass of Kool- Aid(a))x 100
What is the balanced equation for the experiment hot ice (sodium acetate)? ***For example: The decomposition of the hydrogen peroxide into water and oxygen is catalyzed by the iodide ion. 2 H2O2(aq) → 2 H2O(l) + O2(g) This is what I have but I feel like I am missing something? Na+ [HCO3]- + CH3 - COOH ---> CH3 - COO-NA+ + H2O + CO2
How many grams of Cu(OH)2 will precipitate when excess KOH solution is added to 41.0 mL of 0.618 M CuBr2 solution? CuBr2(aq) + 2KOH(aq) Cu(OH)2(s) + 2KBr(aq)g?
what is the the molar mass of KHP? If a student weighs out 0.614 g of KHP and titrates it with sodium hydroxide solution, what is the molarity of the sodium hydroxide solution of it takes 35.01 mL of it to titrate the KHP?
One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate, solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose an EPA chemist tests a 200. mL sample of groundwater known to be contaminated with cadmium chloride, which would react with silver nitrate solution like this: CdCl2(aq) + 2 AgNO3(aq) → 2 AgCl(s) + Cd (NO3)2(aq) The chemist adds 89.0 mM silver nitrate solution to the sample until silver chloride stops forming. He then washes, dries, and weighs the precipitate. He finds he has collected 5.4 mg of silver chloride. Calculate the concentration of cadmium chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits. E d OL E
Give all answers online to 3 significant figures. 115.0 mL of 0.175 M KOH is mixed with 175.0 mL of 0.150 M NiSO4.(a) Write a balanced chemical reaction for the reaction that occurs. (b) The mass of precipitate that forms is gAt the completion of the reaction,(c) the concentration of nickel ions in solution would be M, and(d) the concentration of the sulphate ions would be M
The balanced chemical equation for the reaction between calcium hydroxide and hydrochloric acid is: Ca(OH)2 ( aq) + 2 HC1 ( aq )→ CaCl2 ( aq ) + 2 H,0 (1) We can interpret this to mean: 1 mole of calcium hydroxide and |mole(s) of hydrochloric acid React to produce: | mole(s) of calcium chloride and |mole(s) of water
One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose an EPA chemist tests a 250. mL sample of groundwater known to be contaminated with iron(III) chloride, which would react with silver nitrate solution like this: FeCl,(aq) + 3 AgNO3(aq) 3 AgCl(s) + Fe(NO,),(aq) → The chemist adds 17.0 mM silver nitrate solution to the sample until silver chloride stops forming. He then washes, dries, and weighs the precipitate. He finds he has collected 8.2 mg of silver chloride. Calculate the concentration of iron(III) chloride contaminant in the original groundwater sample. Round your answer to 2 significant digits. mg L
What quantity in moles of precipitate will be formed when 219.5 mL of 0.350 M NaCl is reacted with excess Pb(NO:)2 in the following chemical reaction? 2 NaCl(aq) + Pb(NO:):(aq) → PbCl:(s) + 2 NaNO:(aq)
Complete the balanced molecular chemical equation for the reaction below. If no reaction occurs, write NR after the reaction arrow. LiCI(aq) + K:PO:(aq) –
4.106. Aspirin (acetlsalicyclic acid) may be formed from salicyclic acid and acetic acid as follows:C7H6O3 (aq) + CH3COOH (aq) → C9H8O4(s) + H2O(l)Salicyclic acid Acetic Acid Aspirin b. How many mol of aspirin may be produced from 1.00*102 mol mol salicylic acid? c. How many g of aspirin may be produced from 1.00*102 mol salicylic acid? d. How many g of acetic acid would be required to completely with the 1.00*102 mol salicylic acid? e. For the conditions in part (d), how many g of aspirin would form?
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.