Question

Solutions containing aqueous barium nitrate and aquueous zinc sulfate are combined to yield a precipitate of...

Solutions containing aqueous barium nitrate and aquueous zinc sulfate are combined to yield a precipitate of barium sulfate, if the original solution contained 3.5 g of barium nitrate, calculate the mass of precipitate that complete titration should produce.

A.2.67 g

B. 3.12 g

C. 4.44 g

D. 2.4 g

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

The reaction is

Ba(NO3)2(aq) + ZnSO4(aq)   BaSO4(s)  + Zn(NO3)2(aq)

molar mass of Ba(NO3)2 = 261.337 gm/mole

molar mass of  BaSO4  = 233.43 gm/mol

according to reaction 1 mole of Ba(NO3)2 produce 1 mole precipitate of BaSO4 that mean 261.337 gm of Ba(NO3)2 produce 233.43 gm of BaSO4 then 3.5 gm of Ba(NO3)2 produce =

3.5 233.43 / 261.337 = 3.12 gm of BaSO4  

Answer - B . 3.12 g

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
An aqueous solution of barium nitrate is added dropwise to a solution containing 0.10 M sulfate...
An aqueous solution of barium nitrate is added dropwise to a solution containing 0.10 M sulfate ions and 0.10 M fluoride ions. The Ksp value for barium sulfate = 1.1 x 10-10 and the Ksp value for barium fluoride = 1.7 x 10-6 a.) Which salt will precipitate from solution first? b.) What is the minimum [Ba2+] concentration necessary to precipitate the first salt? c.) What is the minimum [Ba2+] concentration necessary to precipitate the second salt? c.) What is...
When aqueous solutions of potassium phosphate and barium nitrate are combined, does a reaction occur? If...
When aqueous solutions of potassium phosphate and barium nitrate are combined, does a reaction occur? If a reaction does occur, write the balanced formula equation, and net ionic equation.
A. Suppose that aqueous solutions of barium nitrate and potassium carbonate are mixed. What is the...
A. Suppose that aqueous solutions of barium nitrate and potassium carbonate are mixed. What is the name of the compound or compounds that precipitate? B. Insoluble sulfide compounds are generally black in color. Which of the following combinations could yield a black precipitate? Check all that apply. Na2S(aq)+KCl(aq) Li2S(aq)+Pb(NO3)2(aq) Pb(ClO3)2(aq)+NaNO3(aq) AgNO3(aq)+KCl(aq) K2S(aq)+Sn(NO3)4(aq) C. Enter the net ionic equation for the reaction of aqueous sodium chloride with aqueous silver nitrate. Express answer as a chemical equation.
1. Consider the reaction when aqueous solutions of sodium hydroxide and nickel(II) acetate are combined. The...
1. Consider the reaction when aqueous solutions of sodium hydroxide and nickel(II) acetate are combined. The net ionic equation for this reaction is: 2. Consider the reaction when aqueous solutions of barium hydroxide and sodium nitrate are combined. The net ionic equation for this reaction is: 3. Consider the reaction when aqueous solutions of barium sulfide and nickel(II) sulfate are combined. The net ionic equation for this reaction is: 4. In the laboratory you are given the task of separating...
100.0 g of an aqueous solution containing lead nitrate and 100.0 g of an aqueous solution...
100.0 g of an aqueous solution containing lead nitrate and 100.0 g of an aqueous solution containing sodium iodide (both solutions at 22.6 C), are mixed in a calorimeterwith a heat capacity of 472 J/C.; thereactants undergo a metathesis reaction that raises thetemperature of the mixture to 24.2 C. Calculate the amount of heat generated by the reaction, correcting for the heat absorbed by the calorimeter and assuming that the specific heat of the reaction solution is the same as...
3) Cerium(IV) sulfate  is used to titrate a solution of iron(II) ions, with which it reacts according...
3) Cerium(IV) sulfate  is used to titrate a solution of iron(II) ions, with which it reacts according to Ce4+(aq) + Fe2+(aq) = Ce3+(aq) + Fe3+(aq) A cerium(IV) sulfate solution is prepared by dissolving 38.14 g of Ce(SO4)2 in water and diluting to a total volume of 1.000 L. A total of 17.82 mL of this solution is required to reach the endpoint in a titration of a 250.0-mL sample containing Fe2+(aq). Determine the concentration of Fe2+ in the original solution. answer:...
1.Calculate the theoretical mass of sodium carbonate that should be produced by heating 1.678 g of...
1.Calculate the theoretical mass of sodium carbonate that should be produced by heating 1.678 g of sodium bicarbonate. 2.If 1.018 grams of sodium carbonate were produced from the sodium bicarbonate in question 1, calculate the percent yield for the bicarbonate decomposition reaction. 3.A classic high school lab experiment involves combining a solution of barium nitrate, Ba(NO3)2, with a sodium sulfate solution, Na2SO4, forming a precipitate of barium sulfate. Ba(NO3)2(aq) + Na2SO4(aq) ---> BaSO4(s) + 2NaNO3(aq) a. Identify the hazards associated...
A). To what volume should you dilute 121 mL of an 8.00 M CuCl2 solution so...
A). To what volume should you dilute 121 mL of an 8.00 M CuCl2 solution so that 52.0 mL of the diluted solution contains 4.44 g CuCl2? B). Silver nitrate solutions are often used to plate silver onto other metals. What is the maximum amount of silver (in grams) that can be plated out of 5.1 L of an AgNO3 solution containing 3.4 % Ag by mass? Assume that the density of the solution is 1.01 g/mL. Express your answer...
Calculate the theoretical yield of the solid precipitate. Show your work. mass of CaCl2 =2.0 g...
Calculate the theoretical yield of the solid precipitate. Show your work. mass of CaCl2 =2.0 g Molar mass of CaCl2 = 110.98 g/mol Moles of CaCl2 = 2.0 g * 1 mol/110.98g = 0.018 mol Mass of K2Co3 =2.0 g Molar mass of K2Co3 = 138.205 g/mol Moles of K2Co3 =2.0 g * 1 mol/ 138.205g =0.0145 moles According to balanced equation 1mole of CaCl2 reacts with 1 mole of K2CO3 Thus, 0.018 moles of CaCl2 will react with =...
Two aqueous sulfuric acid solutions containing 20.0 wt% H2SO (SG = 1.139) and 60.0 wt% H2SO...
Two aqueous sulfuric acid solutions containing 20.0 wt% H2SO (SG = 1.139) and 60.0 wt% H2SO (SG = 1.498) are mixed to form a 4.00 molar solution (SG = 1.213). Calculate the mass fraction of sulfuric acid in the product solution. Taking 100 kg of the 20% feed solution as a basis, draw and label a flowchart of this process, labeling both masses and volumes, and do the degree-of-freedom analysis. Calculate the feed ratio (volume 20% solution/volume 60% solution). What...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT