When 150.0 mL of a 0.200 M Ca(NO3)2 (MM = 164.088 g/mol) solution is added to...

When 150.0 mL of a 0.200 M Ca(NO3)2 (MM = 164.088 g/mol) solution is added to 200.0 mL of a 0.150 M K3PO4 (MM = 212.27 g/mol) solution, what mass of calcium phosphate (MM = 310.17 g/mol) will precipitate?

a. 9.31 g

b. 3.10 g

c. 2.91 g

d. 1.40 g

e. 4.65 g

Solutions

Expert Solution

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF,...

When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF, CaF2 precipitates, as shown in the net ionic equation below. The initial temperature of both solutions is 25.00°C. Assuming that the reaction goes to completion, and that the resulting solution has a mass of 100.00 g and a heat capacity the same as water, calculate the final temperature of the solution. Ca2+(aq) + 2 F-(aq) → CaF2(s) ΔH° = –11.5 kJ When trying to...

When 50.0 mL of 0.900 M Ca(NO3)2 is added to 50.0 mL of 1.80 M NaF,...

When 50.0 mL of 0.900 M Ca(NO3)2 is added to 50.0 mL of 1.80 M NaF, CaF2 precipitates, as shown in the net ionic equation below. The initial temperature of both solutions is 30.00°C. As the reaction proceeds, the temperature rises to 31.50 °C. Assuming that the reaction goes to completion, and that the resulting solution has a mass of 100.0 g and a specific heat of 4.18 J/(g ∙ °C), calculate the ΔH° for this reaction, expressed in kJ/mol...

When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF,...

When 50.0 mL of 0.400 M Ca(NO3)2 is added to 50.0 mL of 0.800 M NaF, CaF2 precipitates, as shown in the net ionic equation below. The initial temperature of both solutions is 30.00°C. Assuming that the reaction goes to completion, and that the resulting solution has a mass of 100.00 g and a specific heat of 4.18 J/(g ∙ °C), calculate the final temperature of the solution. Ca2+(aq) + 2 F-(aq) → CaF2(s) ΔH° = -11.5 kJ 30.55°C...

A solution is prepared by mixing 150.0 mL of 0.200 M Mg2+ and 250.0 mL of...

A solution is prepared by mixing 150.0 mL of 0.200 M Mg2+ and 250.0 mL of 0.100 M F-. A precipitate forms. Calculate the concentrations of Mg2+ and F- at equilibrium. Ksp = 6.4 × 10-9

If 42.8 mL of 0.200 M HCl solution is needed to neutralize a solution of Ca(OH)2,...

If 42.8 mL of 0.200 M HCl solution is needed to neutralize a solution of Ca(OH)2, how many grams of Ca(OH)2 must be in the solution?

a) Does a precipitate form when 0.200 L of 0.15 M Ca(NO3)2 is mixed with 0.100...

a) Does a precipitate form when 0.200 L of 0.15 M Ca(NO3)2 is mixed with 0.100 L of 0.120 M NaF? At experimental temperature, Ksp of CaF2 = 3.9 x 10-11 b) Calcium hydroxide, Ca(OH)2, is an important component of many mortars, plasters and cements. Calculate the molar solubility of Ca(OH)2 in water if Ksp is 6.5 x 10-6. c) What is the solubility of Ca(OH)2 in a 0.20 M solution of Ca(NO3)2? Ksp of Ca(OH)2 is 6.5 x 10-6

what mass of Ca(NO3)2 must be added to 1.0 L of a 1.0 M HF solution...

what mass of Ca(NO3)2 must be added to 1.0 L of a 1.0 M HF solution to begin precipitation of CaF2. You may assume no volume change on the addition of Ca(NO3)2. Ksp for CaF2 = 4.0 x 10-11 and ka for HF=7.2 x 10-4.

A solution is 3.24 M NH3 (MM 17.04 g/mol) in water (MM 18.02 g/mol). The density...

A solution is 3.24 M NH3 (MM 17.04 g/mol) in water (MM 18.02 g/mol). The density of the resulting solution is 0.974 g/mL. What is the mole fraction, mass percent and molality of NH3 in the solution?

A 0.148-M solution of X (Mm = 177 g/mol) has a density of 1.156 g/ml. What...

A 0.148-M solution of X (Mm = 177 g/mol) has a density of 1.156 g/ml. What is the molality of X in the solution?

A 25.00 mL solution containing 0.3000 M Na2C2O4 (sodium oxalate) was titrated with 0.1500 M Ca(NO3)2...

A 25.00 mL solution containing 0.3000 M Na2C2O4 (sodium oxalate) was titrated with 0.1500 M Ca(NO3)2 to precipitate calcium oxalate: Use Excel to draw a graph of pCa vs. VCa from 0 to 75 mL, using a suitable resolution to show a sharp endpoint. Label the axes and show where the end point lies.

Subjects