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You should use NO MORE THAN 100 mL 0.25 M NH4OH, 4 g Ca(NO3)2· 4H2O, and/or...
You should use NO MORE THAN 100 mL 0.25 M NH4OH, 4 g Ca(NO3)2· 4H2O, and/or 3 g (NH4)2HPO4. NOTE: This is not a stoichiometric recipe. Part of the grading for this lab will be based on your ability to determine appropriate quantities of each reactant. Clearly show the actual amount of each reactant you intend to use. Determine the mass or volume of each reactant in the proper stoichiometric ratio, to synthesize and analyze a sample of calcium hydroxyapatite. The unbalanced equation for the reaction is: H3O+(aq) + Ca(NO3)2(s) + (NH4)2HPO4(s) + NH3(aq) --> Ca10(PO4)6(OH)2(s) + NH4NO3(aq)
Solutions
Amanda K answered 2 years agoRelated Solutions
How many grams of CaF2 will be soluble in 100 ml of 0.250 M Ca(NO3)2? (Ksp...
How many grams of CaF2 will be soluble in 100 ml of 0.250 M
Ca(NO3)2? (Ksp of CaF2 = 3.90*10^-11)
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
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 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!
2 HNO3(aq) + Ca(OH)2(aq) → Ca(NO3)2(aq) + 2 H2O(l) A 350 mL sample of 0.276 M...
2 HNO3(aq) + Ca(OH)2(aq) → Ca(NO3)2(aq) + 2 H2O(l)
A 350 mL sample of 0.276 M HNO3 is partially neutralized by 125
mL of 0.120 M Ca(OH)2. Find the concentration of H+ (aq) in the
resulting solution.
A. 0.210 M
B. 0.00632 M
C. 0.203 M
D. 0.0240 M
E. 0.140 M
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.
Calculate the molar solubility of Ca(IO3)2 in a) 0.060 M Ca(NO3)2 b) 0.060 M NaIO3
Calculate the molar solubility of Ca(IO3)2
in
a) 0.060 M Ca(NO3)2
b) 0.060 M NaIO3
How many moles of NH4Cl must be added to 100 mL of 0.1 M NH4OH solution...
How many moles of NH4Cl must be added to 100 mL of
0.1 M NH4OH solution to prevent precipitation
of Mn(OH)2 when this solution is added to 100 mL of a
0.002 M solution of MnCl2? Assume no change
involume on addition of NH4Cl.
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