Determine the mass of sodium phosphate required to prepare
100.00 mL of a 0.500 M solution....
Determine the mass of sodium phosphate required to prepare
100.00 mL of a 0.500 M solution. Solid sodium phosphate, Na3PO4,
will be provided; it has a formula weight of 163.94 g/mol.
*Calculate the mass of sodium acetate (CH3COONa) required to
prepare 50 mL of a 0.10 M sodium acetate solution. Show work.
Verify that this matches the amount you place into cup #3 in
Activity 1.
*Calculate the volume of 6 M acetic acid needed to prepare 100
mL of a 0.10 M acetic acid (CH3COOH) solution. Show work.
*Calculate the volume of 1 M sodium hydroxide (NaOH) needed to
prepare 10 mL of a 0.10 M sodium hydroxide solution. Show...
use the Henderson-Hasselbalch equation to determine how to
prepare 100 mL of 0.10 M sodium phosphate pH 6.80 and another
solution of pH 7.70. The apparent pKa of phosphate is 6.77.
Calculate the mass of ammonium chloride required to prepare 25
mL of a 2.0 M solution, and the mass of calcium chloride required
to prepare 25 mL of a 2.0 M solution.
when 23.8ml of 0.0985 M sodium
phosphate solution is combined with 18.2 ml of 0.0105M copper (II)
sulfate solution the precipitation reaction results in the
formation of insoluble Copper(II) phosphate
a.) write a balanced molecular
equation, total ionic and net ionic equations and idebtify the
soectatir ions
b.) identify limiting
reagent
c. calculate theoretical yield
in grams of copper (II) phosphate
d.) what is the percent yield
of the reaction if the actual amount of solid formed is
0.227g?
Calculate the mass of CaCO3 required to prepare 500
mL of a standard solution that is 100 ppm in Ca2+.
(Include units and use an appropriate number of sig figs.)
Calculate the mass of NaCl required to prepare 500 mL of a
standard solution that is 100 ppm in Na+.
(Include units and use an appropriate number of sig figs.)
A. What is the molarity of sodium ions in a solution prepared by mixing 202.1 ml of 0.63 M sodium phosphate with 239 ml of 1.31 M sodium sulfide. Enter to 2 decimal places.B. A 17.3 ml sample of a 1.49 M potassium chloride solution is mixed with 58.6 ml of a 1.34 M lead(II) nitrate solution and a precipitate forms. The solid is collected, dried, and found to have a mass of 0.5 g. What is the percent yield?...
Determine the values required to prepare 50.0 mL of a solution
that buffers at a pH of 4.74.
1. Volume of 0.10 M Acetic Acid needed?
2. Volume of 0.1 M sodium Acetate needed?
3. Volume of 1.0 M Acetic Acid needed?
4. Volume of 1.0 M Sodium Acetate needed?
29.7 mL of 4.6 M Sodium Phosphate is mixed with 72.0 mL of 4.0 M
Calcium Bromide to form a precipitate. What precipitate is formed
in this reaction? Calculate the theoretical mass (in grams) of the
precipitate using only the volume and molarity of the Sodium
Phosphate.Calculate the theoretical mass (in grams) of the
precipitate using only the volume and molarity of the Calcium
Bromide.What is the theoretical yield (in grams) of the
precipitate?What is the concentration (in M) of...