What is the molarity of Mg(NO3)2 in a solution resulting from mixing 150 mL of 0.020...

What is the molarity of Mg(NO3)2 in a solution resulting from mixing 150 mL of 0.020 M HNO3 with 150 mL of 0.010 M Mg(OH)2?

Expert Solution

HNO3 millimoles = 150 x 0.020 = 3

Mg(OH)2 millimoles = 150 x 0.01 = 1.5

2HNO3 + Mg (OH)2 ----------------------------> Mg(NO3)2 + 2H2O

3 1.5 0 0 -----------------------> initial

0 0 3 3 ----------------------> after reaction

millimoles of Mg(NO3)2 = 3

molarity of Mg(NO3)2 = 3 / total volume

= 3 / (150+150)

= 3 /300

= 1/100

= 0.01 M

Mg(NO3)2 molarity = 0.01 M

queen_honey_blossom answered 2 years ago

A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO3)2 with 50.0 mL of...

A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO3)2 with 50.0 mL of 0.50 M Co(NO3)2. Sodium hydroxide is then added to the mixture. Assume no change in volume. Ksp = 2.2 × 10-20 for Cu(OH)2, Ksp = 1.3 × 10-15 for Co(OH)2 The hydroxide concentration at which the first metal hydroxide will just begin to precipitate is __________M Using the integer designators, the metal hydroxide that precipitates first is {(1) Cu(OH)2 or (2) Co(OH)2 } _____________M...

A solution is prepared by mixing 50 mL of 1 M Pb(NO3)2 and 75 mL of...

A solution is prepared by mixing 50 mL of 1 M Pb(NO3)2 and 75 mL of .5 M NaF. Calculate the concentration of F- ions present at equilibrium. (Hint: First, write and balance the double displacement reaction taking place between Pb(NO3)2 and NaF to form PbF2(s). Perform the necessary stoichiometry (including finding which reactant is limiting) to calculate how much of each reactant remains after the reaction goes to completion. Remember that stoichiometry has to be done in moles. Once...

A solution is prepared by mixing 100 mL of .01 M Pb(NO3)2 and 100 mL of...

A solution is prepared by mixing 100 mL of .01 M Pb(NO3)2 and 100 mL of .001 M NaF. Will PbF2(s) precipitate in this reaction? Calculate the concentration of F- ions present at equilibrium. PbF2(s) <--> Pb2+(aq) + 2F-(aq) Kc= 3.7E-8 Please show all work! Thank you!

What will the molarity be of the resulting solutions made by mixing the following? Assume that...

What will the molarity be of the resulting solutions made by mixing the following? Assume that volumes are additive. a)116 mL of 3.6 M H3PO4 with 776 mL of H2O (b) 219 mL of 0.39 M Na2SO4 with 737 mL of H2O (c) 75 mL of 0.50 M HNO3 with 75 mL of 1.5 M HNO3

Consider the mixing of 3.05 mL of 0.220 M Mg(NO3)2 and 1.00 L of 0.180 M...

Consider the mixing of 3.05 mL of 0.220 M Mg(NO3)2 and 1.00 L of 0.180 M K3PO4. (a) Write a balanced chemical equation that describes the double displacement reaction between these solutions. (Include states-of-matter under the given conditions in your answer.) (b) Calculate how many grams of the precipitate will form. What would be the concentration of a solution made by diluting 46.9 mL of 4.54 M KOH to 625 mL?

3. What is the pH of the resulting solution after 150 mL of a 3.2 M...

3. What is the pH of the resulting solution after 150 mL of a 3.2 M sodium hydroxide solution is mixed with 4.0 mL of a 4.0 M vinegar solution? 4. In the above question is the acid or base a limiting reagent? 5. Calculate the pH after adding 40.0 mL of 3.7 M potassium hydroxide to 20.0 mL of 12 M formic acid. 6. How many more mL of the 3.7 M potassium hydroxide solution must be added to...

A 23.33-mL solution containing 1.718 g Mg(NO3)2 is mixed with a 30.50-mL solution containing 1.467 g...

A 23.33-mL solution containing 1.718 g Mg(NO3)2 is mixed with a 30.50-mL solution containing 1.467 g NaOH. Calculate the concentrations of the ions remaining in solution after the reaction is complete. Assume volumes are additive. If a species fully precipitates, type 0. a.) ______ M Mg2+ b.) ______ M NO3- c.) ______ M Na+ d.) ______ M OH-

Question

What is the molarity of Mg(NO3)2 in a solution resulting from mixing 150 mL of 0.020...

Solutions

Expert Solution

Related Solutions