A solution is made by mixing 13.5 g of Sr(OH)2 and 75.0 mL of 0.150 M...

Question

Question

A solution is made by mixing 13.5 g of Sr(OH)2 and 75.0 mL of 0.150 M HNO3. Calculate the concentration of Sr2+ ion remaining in solution.

Calculate the concentration of Sr2+ ion remaining in solution.

science chemistry

Answer 1

Answer #1

Answer: Concentration of Sr²⁺ remaining in the solution = 1.40 M

Answer 2

Similar Homework Help Questions

A solution is made by mixing 75.0 ml of 0.350 M BaCl_2 with 30.0 ml of...

A solution is made by mixing 75.0 ml of 0.350 M BaCl_2 with 30.0 ml of 0.800 M LiCl. What is the molar concentration of the chloride ion in the new solution?
What is the pH of a solution made by mixing 1.10 mL of 0.0058 molar Sr(OH)2...

What is the pH of a solution made by mixing 1.10 mL of 0.0058 molar Sr(OH)2 with 9.00 mL of 0.0036 molar Sr(OH)2 solution?
10. Calculate the pH of a solution made by mixing 40.0 mL of 0.150 M ammonia...

10. Calculate the pH of a solution made by mixing 40.0 mL of 0.150 M ammonia with 10.0 mL of 0.100 M HCl

O.I44 32. What is the pH of a 0.150 M Sr(OH)2 solution? (2

O.I44 32. What is the pH of a 0.150 M Sr(OH)2 solution? (2
68.5 mL of a HNO3 solution with unknown concentration is titrated with 0.150 M KOH solution....

68.5 mL of a HNO3 solution with unknown concentration is titrated with 0.150 M KOH solution. The end point is reached after 25 m/L of KOH solution is added. what is the molarity of the HNO3 solution ? 1 р . HNO3 + KOH --> KNO3 + H20 68.5 mL of a HNO3 solution with unknown concentration is titrated with 0.150 M KOH solution. The endpoint is reached after 25.0 mL of KOH solution is added. What is the molarity...
31. When 75.00 mL of 0.1500 M Silver nitrate and 75.0 mL of 0.150 M HCl...

31. When 75.00 mL of 0.1500 M Silver nitrate and 75.0 mL of 0.150 M HCl are mixed in a constant-pressure calorimeter, the temperature of the mixture increases from 22.00 °C to 24.11 °C. The temperature increase is caused by the following reaction: AgNO3(aq) + HCl(aq) AgCl(s) + HNO3(aq) Calculate AH for this reaction in silver nitrate, assuming that the combined solution has a mass of 150.0 g and a specific heat of 4.184 J/g °C. A. -128.00K) B. 128.00...

31. When 75.00 mL of 0.1500 M Silver nitrate and 75.0 mL of 0.150 M HC)...

31. When 75.00 mL of 0.1500 M Silver nitrate and 75.0 mL of 0.150 M HC) are mixed in a constant-pressure calorimeter, the temperature of the mixture increases from 22.00 °C to 24.11 °C. The temperature increase is caused by the following reaction: AgNO3(aq) + HCl(aq) → AgCl(s) + HNO3(aq) Calculate AH for this reaction in silver nitrate, assuming that the combined solution has a mass of 150.0 g and a specific heat of 4.184 J/g °C. A. -128.00KJ B....
Indicate the concentration of each ion present in the solution formed by mixing the following. A....

Indicate the concentration of each ion present in the solution formed by mixing the following. A. 42.0 mL of 0.150 M NaOH and 37.6 mL of 0.410 M NaOH. Assume that the volumes are additive. B. 44.0 mL of 0.140 M Na2SO4 and 25.0 mL of 0.160 M KCl. Assume that the volumes are additive. C. 3.20 g KCl in 75.0 mL of 0.220 M CaCl2 solution. Assume that the volumes are additive.
25.0 mL of 0.150 M Na3PO4 are combined with 25.0 mL of 0.200 M Sr(NO3)2. Calculate...

25.0 mL of 0.150 M Na3PO4 are combined with 25.0 mL of 0.200 M Sr(NO3)2. Calculate the concentrations of all ionic species (except H+ and OH-) at equilibrium. Ksp( Sr3(PO4)2 ) = 1.0x10^-31. Answer: Na+ = 0.225 M PO4= 0.0084 M Sr= 1.12 x 10^-9 M NO3 = 0.220 M

Calculate the hydrogen ion concentration in mol/L for a solution Sr(OH)2 of concentration 0.017 M

Calculate the hydrogen ion concentration in mol/L for a solution Sr(OH)2 of concentration 0.017 M