Question

A 1.25 g sample of NaHCO_{3} is dissolved in 150.0 mL of
water. Calculate the molarity of this solution.

Answer #1

8.8430 g of FeCl3 are dissolved in 150.0 mL of water. What is
the concentration of FeCl3 (in M) in resulting the solution? (FeCl3
is 162.206 g/mol) [FeCl3] = ___ M

What is the molarity of each solution?
39 g of KCl dissolved in enough water to give
375 mL of solution.
85.8 g of sucrose,
C12H22O11, dissolved in enough
water to give 725 mL of solution.
8.4 g of ammonium sulfate,
(NH4)2SO4, dissolved in enough
water to give 2.35 L of solution.

Calculate the molarity of a solution made by adding 150.0 mL of
water to 85.00 mL of a 0.157 M solution.
How many milliliters of a 0.180 M KCl solution are needed to
provide 0.0306 mol KCl?
If the red dye #40 concentration is 3.00×10-3 M in
the original syrup, what is its concentration in dilution #3 (enter
your answer in the box below the image)? The red dye #40 syrup is
diluted by a factor of 2 three times....

A.
6.7 g of K3PO4 are dissolved in 500 mL of water. What is the
concentration (in normality) of PO4^3- ions in solution?
B. Calculate the formal concentration (in molarity) of a KCl
solution if 18.6 g of KCl are dissolved in 500 mL of water?
C. What NaCl concentration results when 234 mL of a 0.830 M
NaCl solution is mixed with 502 mL of a 0.370 M NaCl
solution?

15.0 grams of NaOH was dissolved in 150.0 ml of 20.0 °C water.
The temperature rose to 25.6 °C. Calculate the ΔH for the
dissociation.

What is the pH when 5.0 g of sodium acetate, NaC2H3O2, is
dissolved in 150.0 mL of water? (The Ka of acetic acid, HC2H3O2, is
1.8×10−5.)

specifically calculate the molarity and molality for hydrogen
chloride gas dissolved in pure water, at 298K, to produce a
hydrochloric acid solution that is 37.0% HCl and density of
solution is 1.19 g/mL
( you have to specific tasks, but how many implied tasks are
there. Problem requires...)
- Find molarity for HCl(aq)
- Find molality for HCl(aq)

When a 5.00 g sample of CaCO3 (at 22.0oC) was dissolved in 125
mL water (density = 1.00g/mL, at 22.0oC) the final equilibrium
temperature of the resulting solution is 32.8oC. Calculate the
enthalpy of solution, ΔHs(kJ/mole ofCaCO3). (Cs-calciumcarbonate=
0.76 J/goC

1a. 8.0102 g CuSO4*5(H2O) is
dissolved to make 100.00 mL solution. What is the
molarity?
Cu= .05M
1b. 3.3079 g Pb(NO3)2 is
dissolved to make 20.00 mL solution. What is the
molarity?
Pb=.05M

A 3.98 g sample of solid NaBr (s) is dissolved in 361 mL of
water in a coffee cup calorimeter. Once all of the NaBr (s) is
dissolved in the water, the final temperature of the solution is
found to be 30.04°C. If the initial temperature of the water in the
calorimeter was 21.84 °C, calculate the calorimeter constant (in
J/K) for the coffee cup calorimeter.
The heat of solvation of NaBr (s) is -0.60 kJ/mol.

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