Gases ____ to fill whatever space is available to them.
100
Calculate the volume of 3.0 M sulfuric acid needed to prepare the dilution.
Describe how you would prepare 1.0 L of a 0.10 M solution of sulfuric acid from a 3.0 M solution of sulfuric acid.
100
pH = - log [H+] = - log(1.61 x 10-3)
Calculate the equilibrium concentrations and pH for a 0.20 M proprionic acid solution. Ka = 1.3 x 10-5
200
262.79g
Find the formula mass of Mg3(PO4)2
200
2.2 E25 atoms H
How many atoms of H are in 2 mol of C8H18?
200
Freezing
The change in a state of matter from a liquid to a solid.
200
Since the solute (phenolphthalein) is a solid, the solution is percent by mass. Mass percent means the number of grams of solute per 100 g of solution.
Describe how you would prepare 100 g of a solution that is 0.5% phenolphthalein by mass.
What is the percentage, by mass, of the H in 2 mol of C8H18?
300
Surface tension
The pull on the surface of liquids that allow liquids to form drops when they fall. (2 words)
300
Calculate the volume of 5.0 M sodium hydroxide needed to prepare the dilution.
Describe how you would prepare 500 mL of a 0.25 M solution of sodium hydroxide from a 5.0 M solution of sodium hydroxide.
300
Using the following equations: pOH = - log [OH-]; pH + pOH = 14
Calculate the Ka for a 0.3 M solution of HA (weak acid) if the pH = 3.65
400
0.112 mol KMnO4
How many moles are in 17.7 g of KMnO4
400
mass of H2O = 2.1555 x 18 = 38.8 g
If 27.3g of C8H18 are combusted, what mass of water will be produced?
400
Liquid
A state of matter that has no fixed shape but that has a definite volume.
400
Calculate the volume of 85.0% phosphoric acid needed.
Describe how you would prepare 500 mL of a 1.0 M solution of phosphoric acid from 85.0% phosphoric acid that is pure. The gram formula weight of phosphoric acid is 98.00 g/mol, and the density of 85.0% phosphoric acid is 1.685 g/mL.
400
Complete the equilibrium and express the equilibrium concentrations in terms of a single unknown 'x'.
Calculate the pH for a 0.2 M pyridine solution. Kb = 2.0 x 10-9
500
0.079 mol C12H22O11
How many moles are in 26.9g of C12H22O11
500
Faster
Particles in a gas are ____ apart than the particles in a liquid.
500
Calculate the mass of impure potassium chloride needed.
Describe how you would prepare 500 mL of a 1.0 M solution of potassium chloride that is 93.0% pure. The gram formula weight of potassium chloride is 74.56 g/mol.
500
This is done the same way as problem 1, using a Ka value of 4.2 x 10-7
Calculate the equilibrium concentrations and pH for a 0.20 M carbonic acid solution. Compare the answer to problem 1. Note which has the higher Ka and lower pH. Ka = 4.2 x 10-7