Molarity/stock solution
What mass of HCL is in 325 mL of 0.12M HCl.
1.42g
When Manganese(IV) oxide reacts with aluminum metal, aluminum oxide, and manganese metal form. Write a Balanced equation for this reaction and calculate the mass of aluminum metal required to completely react with 75.0g of manganese(IV) oxide
31.0g
Write the complete ionic equation for the reaction between potassium phosphate and aluminum sulfate. Sum the coefficients including implied 1’s for your final answer.
24
Write the balanced equation for the reaction between nitric acid and sodium sulfite.
2HNO3(aq)+ Na2SO3(aq) -> H2O(l) +SO2(g)+ 2NaNO3(aq)
What is the oxidation state for Ca in CaF2
2+
What volume (in mL) of 0.155 M nitric acid is needed to neutralize 1.89 g of calcium hydroxide?
329 ml
Octane (C8H18) produces 178g and Oxygen produces 525g. What mass remains of the excess reactant? Hint: Create a Balanced Equation
28g excess
Write a complete ionic equation to show the reaction of aqueous lead(II) nitrate with aqueous potassium sulfate to form solid lead(II) sulfate and aqueous potassium nitrate.
11
Write the balanced equation for the reaction between perchloric acid and lithium carbonate.
2HClO4(aq)+ Li2CO3(aq)-> H2O(l)+CO2(g)+2LiClO4
Is this reaction below a redox reaction, If so, state which is an oxidizing agent, and the reducing agent.
Mg(s) + Fe2+ (aq)-> Mg2+(aq)+ Fe(s)
Yes
Mg is reducing agent
Fe is the oxidizing agent
What is the concentration of chloride ions in a solution made from 25.0g of CaCl2 and enough water to make 100.0 ml of Solution.
4.51 M
Iron(III) oxide reacts with carbon monoxide to form iron metal and carbon dioxide. A container initially has 48.55 grams of iron(III) oxide and 32.80g of carbon monoxide. Write a balanced equation and then calculate the mass of excess reactant that remains after the reaction goes to completion.
7.25g excess
Write the complete ionic equation for the reaction between silver nitrate and ammonium bromide. Sum the coefficients including implied 1’s for your final answer.
7
The titration of 10.50 mL of an unknown sulfuric acid solution requires 18.2 mL of 0.225 M potassium hydroxide solution to reach the equivalence point. What is the concentration of the unknown acid sample? Hint: Write a balanced equation for the reaction!
0.195
Classify each change if it is physical or chemical
Natural gas burns in a stove.
Liquid propane in a gas grill evaporates because the valve was left open.
Liquid propane in a gas grill burns in a flame.
A bicycle frame rusts on repeated exposure to air and water.
chemical
physical
chemical
chemical
You add 5.0 mL of a 15M HNO3 solution to some water in a volumetric flask and dilute the solution to 200.0 mL. What is the concentration of the new HNO3 solution?
0.375M
Urea (CH4N2O) is a common fertilizer that is synthesized by the reaction of ammonia (NH3) with carbon dioxide: 2NH3(aq)+ CO2(aq)-> CH4N2O(aq) + H2O(l). In an industrial synthesis of urea, a chemist combines 136.4kg of ammonia with 211.4kg of carbon dioxide to obtain 168.4kg of urea. Determine the limiting reactant, theoretical yield of urea, and percent yield.
limiting reactant: NH3,
theoretical yield: 240,5kg of CH4N2O.
Percent yield: 70.01%
Write balanced net ionic equations for each acid-base reaction.
HBr(aq)+ NaOH(aq)->
HF(aq)+ NaOH(aq)->
HC2H3O2(aq)+ RbOH(aq)->
H+(aq) + Oh-(aq)-> H2O(l)
HF(aq)+ OH-(aq)-> H2O(l)+ F-(aq)
HC2H3O2(aq)+ OH-(aq)-> H2O(l) + C2H3O2- (aq)
A 30.00 mL sample of an unknown phosphoric acid solution is titrated with a 0.200 M KOH solution. The equivalence point is reached when 26.38 mL of KOH solution is added. What is the concentration of the unknown phosphoric acid solution?
HINT: Write a balanced equation first!
0.0586M
C+ H2SO4-> CO2+ SO2+ H2O
What is oxidized and reduced in this equation
C is oxidized
S is reduced
A student prepared a stock solution by dissolving 125.0g of solid sodium phosphate in enough water to make 500 mL of solution. What volume of this sodium phosphate stock solution is needed to create 250.0 mL of solution with a sodium ion concentration of 0.600M?
32.8 mL
Write a balanced equation for the complete combustion of methanol, CH3OH. If the % yield is 85.2% and 426g of water were produced, how many grams of methanol were combusted in the presence?
445g
Complete and balance each acid-base equation
H2SO4(aq)+ Ca(OH)2 (aq) ->
HClO(aq)+ KOH(aq)->
H2SO4(aq)+ NaOH(aq)->
H2SO4(aq)+ Ca(OH)2 (aq) -> H2O(l) +CaSO4 (s)
HClO(aq)+ KOH(aq)-> H2O(l)+ KClO4(aq)
H2SO4(aq)+ NaOH(aq)->2H2O(l)+Na2SO4(aq)
A 2.20 g sample of an unknown acid (empirical formula = C3H4O3) is dissolved in 1.0 L of water. A titration required 12.5 mL of 0.500 M Ba(OH)2 to react completely with all the acid present. Assuming the unknown acid has one acidic proton per molecule, what is the molecular formula of the unknown acid?
C6H8O6
Classify each property as a physical or chemical.
the tendency of ethyl alcohol to burn
the shine of silver
the odor of paint thinner
the flammability of propane gas.
chemical
physical
physical
chemical