Question
In: Chemistry
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
queen_honey_blossom answered 2 years agoRelated 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.
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