a) What is the molarity of the solution that was prepared by
dissolving 3.25 g of sulfuric acid in water to a total volume of
500.0 mL?
b)What is the molarity of the hydrogen ion in part a if you
assume the sulfuric acid ionizes completely? Write a balanced
chemical equation.
Question 17 # Determine the molarity of a solution formed by
dissolving 168.2 g of Ki (molar mass of Ki 165996) in enough water
to yield 401.5mL of solution Answer with 4 significant figures.
Question 18# How many milliers of a concentrated 5.00 M KNO,
solution are required to make 100.0 ml of a diluted 0.201M KNO,
solution Answer with 3 significant figures.
A solution is obtained by dissolving 171.2 g of sucrose (i = 1)
with 360.4 g of H 2 O at 55 ºC. Sucrose is a
non-volatile solute.
The water vapor pressure at 55ºC is 118.1 torr. The molar mass
of sucrose is 342.3 g / mol and H 2 O is 18.02 g /
mol.
To calculate the mole fraction, it is necessary to calculate
the total moles . The result of this
computation is:
Calculate the vapor pressure on...
1. Calculate the molarity of a solution made by dissolving
0.4000 g of acetylsalicylic acid (180.15 g/mol) in 250.00 mL of
water.
2. Calculate the volume of the solution prepared in (1) needed
to make 100.00 mL of solution with a concentration of 4.00 x 10–4
M.
3. What are the correct units for molar absorptivity according
to Beer’s Law?
4. Describe how you will determine the concentration of
acetylsalicylic acid in your individual diluted aspirin-tablet
solutions. (Hint: Think Beer’s...
What is the molality and molarity of solution prepared by
dissolving 35.0 mL of benzene (density = 0.877 g/mL) in 175 mL of
hexane (density = 0.660 g/mL)? Assume volumes are additive.
1. What is the molarity of a solution of NaOH if 23.4 mL
required to neutralize 25 mL of 0.25M H2SO4?
2.What is the pH of a solution produced by dissolving 1.5g HCI
to make 1L of solution?
Please help, step by step solutions .. thanks!
3)Suppose a solution is prepared by dissolving 15.0 g NaOH in
0.150 L of 0.250 M nitric acid. What is the final concentration of
OH- ions in the solution after the reaction has gone to completion.
Assume that there is no volume change when adding the grams of
NaOH.
A solution was produced by dissolving NH3 to give a 250. mL
solution with 3.00 M NH3. a. What is the pH of this solution? pH
=
b. What mass of NH4Cl must be added to this solution to give a
pH of 9.45? __ g
c. If 40. mL of 2.0 M KOH was added to this solution, what will
be the pH of this solution? pH =
d. If 40. mL of 2.0 M KOH was added to...