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Electrolytes & Solubility
Reaction Types & Equations
Solution Calculations
Redox & Activity
A bit of everything
100

This is the term for a substance that dissolves in water but does not produce ions and therefore does not conduct an electric current.

non-electrolyte

100

The reaction between an aqueous acid and an aqueous base that produces water and a salt is known by this specific type of metathesis reaction.

acid-base neutralization

100

This is the standard unit for volume that must be used when calculating molarity (mol/L)

Liter (L)

100

In the H2SO4 molecule, this is the oxidation number of sulfur. 

+6

100

This is the final concentration ( M) of HCl when you combine 1.50L of  4.00M HCl with 2.25L of 3.00M HCl

3.40 M

200

When ethanol, CH3CH2OH, is placed in water, it is classified as this specific type of electrolyte

non-electrolyte

200

This term describes the ions present in a complete ionic equation that do not participate in the actual chemical reaction and are omitted from the net ionic equation.

spectator ions

200

When calculating molarity for a 750. mL solution, you must first convert the volume to liters by dividing by this number.

1,000

200

This table is used to predict if a metal like Magnesium will displace Hydrogen from an acid.

Activity Series

200

In the reaction between Aluminum metal (Al) and Copper(II) Nitrate (Cu(NO3)2), this is the balanced coefficient for the Copper solid product.

3

2Al + 3Cu(NO3)2 -> 3Cu + 2Al(NO3)3

300

Ammonia (NH3) is a weak base, meaning it is this specific type of electrolyte in water, only partially ionizing

weak electrolyte

300

When sodium bicarbonate (NaHCO3) reacts with acetic acid (HC2H3O2), this specific gaseous product is formed, indicating a gas evolution reaction.

carbon dioxide (CO2)

300

To find the number of moles of methanol (CH3OH) in 75.0 g, you must divide the mass by this specific molar mass (rounded to two decimal places)

32.04 g/mol

300

In a redox reaction, this term describes the loss of electrons, which causes the oxidation number to increase

Oxidation

300

What is the concentration (M) of a 25.00mL H2SO4 solution that is neutralized by 44.47 ml of 2.500M NaOH, accounting for the 1:2 mole ratio.

2.224 M

Show Work: 

Convert mL to L

44.47mL -> 0.04447L

convert to moles

0.04447L NaOH * 2.500 mol/L =0.11 moles

Stoichiometry

0.11 moles NaOH * 1mol H2SO4 / 2mol NaOH = 0.056 Moles

Molarity = Moles/L

0.056 Moles / 0.025L (converted to L it was given in the problem) = 2.224M

400

TRUE/FALSE

According to the solubility guidelines, salts containing the nitrate ion (NO3-) are always soluble with no known exceptions

True

400

For the reaction 3Ca(OH)2(aq) + 2H3PO4(aq) → 6H2O(l) + Ca3(PO4)2(s), these two substances are the products included in the net ionic equation.

water (H2O) and calcium phosphate [Ca3(PO4)2]


400

what is the final concentration (M) if 1.50 L of 0.100 M NaCl is diluted to a total volume of 3.50 L

0.0429

Show work:

eq: M1V1=M2V2 ->M2=(M1 V1)/V2

Known

M1=0.100M NaCl

V1= 1.50L

M2= ?

V2= 3.50L


400

According to the Activity Series, this is the result when solid Copper is added to HCl (aq)

NR (No Reaction)

400

In the reduction of the permanganate ion (MnO4-) to Mn2+, this is the total change in the oxidation number of Manganese, indicating the number of electrons gained.

5 

Show Work:

MnO4- (Mn oxidation# = +7) 

Mn2+ (Mn oxidation # = +2)

(+7)-(+2) =5

500

When solutions of silver nitrate (AgNO3) and lithium bromide (LiBr) are mixed, this specific insoluble precipitate is formed, consistent with the solubility rules 

silver bromide (AgBr)

500

When writing the ionic equation for the reaction between K2CO3 and BaCl2, which product is a solid(s) ?

barium carbonate (BaCO3)

500

This is the volume of 2.00 M HCl required to neutralize 35.6 mL of 1.95 M NaOH


34.7mL

Show Work:

1) Stoichiometry

Balanced eq: HCl(aq) + NaOH(aq) -> H2O(l) + NaCl(aq)

1mol HCl = 1mol NaOH

2) Find Moles of NaOH present

1.95moles/L * 0.0356L = 0.07moles NaOH

3) Solve for moles of HCl needed

Moles are the same so 0.07 moles HCl needed

Volume= (moles/molarity)

Molarity given in the equation and now we know moles

0.07 moles / 2M (moles/L) = 0.0347 L -> 34.7 ml (moles cancel out leaving liters then convert it if you want to)

500

This is the oxidation number of Nitrogen in the nitrate anion (NO3-). 

+5

500

In a redox reaction between Zn(s) and AgNO3(aq), this is the total number of electrons transferred in the balanced net ionic equation.

2

2 Zn+ 2 Ag+ -> Zn2+ + 2 Ag