The formula weight of LiClO4 is ________ amu.
106.3
1 mole of which of the following will have the largest mass?
gold
The formula weight of lead nitrate (Pb(NO3)2) is ________ amu.
331.2
There are ________ sulfur atoms in 25 molecules of C4H4S2.
50
The formula weight of a substance is ________.
the sum of the atomic weights of each atom in its chemical formula
The formula weight of silver chromate (Ag2CrO4) is ________ amu.
331.73
One mole of ________ contains the smallest number of atoms.
NaCl
Determine the mass percent (to the hundredths place) of C in sodium bicarbonate (NaHCO3).
(/14.30/)
A 30.5 gram sample of glucose (C6H12O6) contains ________ atoms of carbon
6.12 � 1023
Calculate the percentage by mass of nitrogen in PtCl2(NH3)2.
9.34
Pure acetic acid (HC2H3O2) is a liquid and is known as glacial acetic acid. Calculate the molarity of a solution prepared by dissolving 20.00 mL of glacial acetic acid at 25 �C in sufficient water to give 500.0 mL of solution. The density of glacial aceti
0.699
What mass (g) of CaF2 is formed when of NaF is treated with an excess of aqueous calcium nitrate?
0.520
Which combination will produce a precipitate?
Pb(NO3)2 (aq) and HCl (aq)
Oxalic acid is a diprotic acid. Calculate the percent of oxalic acid (H2C2O4) in a solid given that a 0.7984-g sample of that solid required 37.98 mL of 0.2283 M NaOH for neutralization.
48.89
Which of these metals will be oxidized by the ions of cobalt?
iron
The net ionic equation for the reaction between aqueous nitric acid and aqueous sodium hydroxide is ________.
H+ (aq) + OH- (aq) H2O (l)
The reaction between strontium hydroxide and chloric acid produces ________.
a molecular compound and a strong electrolyte
What mass (g) of barium iodide is contained in of a barium iodide solution that has an iodide ion concentration of
19.6
What are the respective concentrations (M) of K+ and PO43- afforded by dissolving 0.800 mol K3PO4 in water and diluting to 1.63 L?
1.44 and 0.491
A 25.5 mL aliquot of HCl (aq) of unknown concentration was titrated with 0.113 M NaOH (aq). It took 51.2 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was ________.
0.227
Which of the following are weak electrolytes?
HNO3
HF
NH3
LiBr
HF, NH3
Oxidation is the ________ and reduction is the ________.
loss of electrons, gain of electrons
What is the formula for phosphoric acid?
H3PO4
Which of these metals is the least easily oxidized?
Na
Au
Fe
Ca
Ag
Au
Which one of the following substances is produced during the reaction of an acid with a metal hydroxide?
H2O
What mass (g) of AgBr is formed when of AgNO3 is treated with an excess of aqueous hydrobromic acid?
4.59
Which combination will produce a precipitate?
KOH (aq) and Mg(NO3)2 (aq)
In the following reaction, which species is reduced?
Au(s) + 3NO3-(aq) + 6H+(aq) Au3+(aq) + NO(g) + 3H2O (l)
H+
N+5
O2-
H2O
Au
N+5
There are ________ mol of bromide ions in 0.500 L of a 0.350 M solution of AlBr3.
0.525
When 0.500 mol of HC2H3O2 is combined with enough water to make a 300.0 mL solution, the concentration of HC2H3O2 is ________ M.
1.67
________ is an oxidation reaction.
Rusting of iron
Based on the activity series, which one of the reactions below will occur?
Mn (s) + NiCl2 (aq) MnCl2 (aq) + Ni (s)
The net ionic equation for the dissolution of zinc metal in aqueous hydrobromic acid is ________.
Zn (s) + 2H+ (aq) Zn2+ (aq) + H2 (g
The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is ________.
H2SO4 (aq) + 2KOH (aq) 2H2O (l) + K2SO4 (aq)
The molarity of a solution prepared by diluting 43.72 mL of 5.005 M aqueous K2Cr2O7 to 500. mL is ________.
0.438
One method for removal of metal ions from a solution is to convert the metal to its elemental form so it can be filtered out as a solid. Which metal can be used to remove aluminum ions from solution?
none of these
What is the concentration (M) of a NaCl solution prepared by dissolving 3.8 g of NaCl in sufficient water to give 245 mL of solution?
(/0.27/)
What volume (mL) of 142 M phosphoric acid can be neutralized with of sodium hydroxide?
211
A 0.100 M solution of ________ will contain the highest concentration of potassium ions.
potassium phosphate
Which one of the following is a weak acid?
HF
Zinc is more active than cobalt and iron but less active than aluminum. Cobalt is more active than nickel but less active than iron. Which of the following correctly lists the elements in order of increasing activity?
Ni < Co < Fe < Zn < Al
How many grams of H3PO4 are in 175 mL of a 4.00 M solution of H3PO4?
68.6
Calculate the concentration (M) of sodium ions in a solution made by diluting 50.0 mL of a 0.874 M solution of sodium sulfide to a total volume of 250.0 mL.
0.350
Which hydroxides are strong bases?
Sr(OH)2
KOH
NaOH
Ba(OH)2
Sr(OH)2, KOH, NaOH, Ba(OH)2
The concentration of sulfate ions in a 0.233 M solution of sulfuric acid is ________.
0.233 M
How many grams of CH3OH must be added to water to prepare 175 mL of a solution that is 1.0 M CH3OH?
/5.6/)
The net ionic equation for formation of an aqueous solution of NiI2 accompanied by evolution of CO2 gas via mixing solid NiCO3 and aqueous hydriodic acid is ________.
NiCO3 (s) + 2H+ (aq) H2O (l) + CO2 (g) + Ni2+ (aq)
Which of the following is soluble in water at 25 �C?
AgNO3
What is the concentration (M) of CH3OH in a solution prepared by dissolving 34.4 g of CH3OH in sufficient water to give exactly 230 mL of solution?
4.67
Which of the following reactions will not occur as written?
Mg (s) + Ca(OH)2 (aq) Ca (s) + Mg(OH)2 (aq)
What are the respective concentrations (M) of Na+ and SO42- afforded by dissolving 0.500 mol Na2SO4 in water and diluting to 1.33 L?
0.752 and 0.376
Which solution has the same number of moles of NaOH as 50.0 mL of 0.100 M solution of NaOH?
100.0 mL of 0.0500 M solution of NaOH
A titration reached the equivalence point when 16.1 mL of was added to of NaOH (aq) of unknown concentration. What is the concentration (M) of this unknown NaOH solution?
0.561
Which one of the following solutions will have the greatest concentration of hydroxide ions?
1.10 M rubidium hydroxide
Of the metals below, only ________ will not dissolve in an aqueous solution containing nickel ions.
aluminum
chromium
barium
tin
potassium
tin
Oxidation and ________ mean essentially the same thing.
corrosion
What are the respective concentrations (M) of Fe3+ and I- afforded by dissolving 0.200 mol FeI3 in water and diluting to 725 mL?
0.276 and 0.828
How many moles of K+ are present in 343 mL of a 1.27 M solution of K3PO4?
1.31
With which ion will the mercury ion form an insoluble salt?
phosphate
Mixing 10.00 mL of an aqueous solution with 10.00 mL of water represents a ________.
twofold dilution
The spectator ions in the reaction between aqueous hydrofluoric acid and aqueous barium hydroxide are ________.
Ba2+ only
An aliquot (28.7 mL) of a KOH solution required 31.3 mL of 0.118 M HCl for neutralization. What mass (g) of KOH was in the original sample?
0.207
What volume (mL) of 7.48 � 10-2 M perchloric acid can be neutralized with 115 mL of 0.244 M sodium hydroxide?
375
When aqueous solutions of ________ are mixed, a precipitate forms.
NiBr2 and AgNO3
The concentration of iodide ions in a 0.193 M solution of barium iodide is ________.
0.386 M
Aqueous potassium chloride will react with which one of the following in an exchange (metathesis) reaction?
lead nitrate
With which of the following will the Potassium ion form an insoluble salt?
Potassium will form soluble salts with all choices.
Of the following elements, ________ is the only one that cannot be found in nature in its elemental form.
Cu
Hg
Au
Ag
Na
Na
The net ionic equation for the reaction between aqueous sulfuric acid and aqueous sodium hydroxide is ________.
H+ (aq) + OH- (aq) H2O( l)
Aqueous solutions of a compound did not form precipitates with Cl-, Br-, I-, SO42-, CO32-, PO43-, OH-, or S2-. This highly water-soluble compound produced the foul-smelling gas H2S when the solution was acidified. This compound is ________.
(NH4)2S