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29 terms

Molarity

STUDY
PLAY
How many moles of gas are contained in a balloon with a volume of 10.0L at STP?
0.446mol
What is the volume occupied by 0.350mol of S02 (g) at STP?
7.84L
What is the volume occupied by 50.0g of NH3 (g) at STP?
65.9L
Calculate the concentration of the solute in mol/L in the diluted solution: 125mL of 0.64M HCl diluted to 2.0L
0.040mol/L
Calculate the concentration of the solute in mol/L in the diluted solution: 25.0mL of 0.22M MgSO4 diluted to 500.0mL
0.11M
Calculate the concentration of the solute in mol/L in the diluted solution: 10.0mL of 4.0M KOH diluted to 5.0L
0.0080M
Calculate the concentration of the solute in mol/L in the diluted solution: 1.00mL of 0.50M NH4Cl diluted to 250.0mL
0.0020M
Calculate the volume required to prepare the diluted solution: Given 6.0M NaOH; need 5.0L of 0.10M NaOH
0.083L
Calculate the volume required to prepare the diluted solution: Given 2.0M HCl; need 0.50L of 0.010M HCl
0.0025L
Calculate the volume required to prepare the diluted solution: Given 1.0M BaCl2; need 125mL of 0.040M BaCl2
0.0050L
Write dissociation equations for each of the solutions and then calculate the concentration of each ion: 0.060M Fe2(SO4)3
0.060M, 0.12M, 0.18M
Write dissociation equations for each of the solutions and then calculate the concentration of each ion: 2.40M Li3PO4
2.40M, 7.20M, 2.40M
Write dissociation equations for each of the solutions and then calculate the concentration of each ion: 0.023M Ca(OH)2
0.023M, 0.023M, 0.046M
Write dissociation equations for each of the solutions and then calculate the concentration of each ion: 1.7M (NH4)3PO4
1.7M, 5.1M, 1.7M
Write dissociation equations for each of the solutions and then calculate the concentration of each ion: 0.42M Mg(ClO3)2
0.42M, 0.42M, 0.84M
Calculate the concentration of each ion in each mixed solution: 2.0L of 0.40M MgS04 mixed with 2.0L of 0.080M Kl
Mg=0.20M, SO4=0.20M, K=0.040M, I=0.040M
Calculate the concentration of each ion in each mixed solution: 3.0L of 0.48M NaOH mixed with 1.0L of 0.32M KOH
Na=0.36M, OH=0.44M, K=0.080M
Calculate the concentration of each ion in each mixed solution: 200mL of 0.6M AlBr3 mixed with 300mL of 0.4M BaBr2
Al=0.24M, Ba=0.24M, Br=1.2M
Calculate the concentration of each ion in each mixed solution: 20.0mL of 0.50M FeCl3 mixed with 80.0mL of 0.15M NH4Cl
Fe=0.10M, NH4=0.12M, Cl=0.42M
Calculate the concentration of each ion in each mixed solution: 6.4g of NaCl and 5.2g of KCl dissolved and made up to 250mL
Na=0.44M, K=0.28M, Cl=0.72M
Calculate the concentration of each ion: 0.24M Al2(SO4)3
0.24M, 0.48M, 0.72M
Calculate the concentration of each ion: 0.6M CrCl3
0.6M, 0.6M, 1.8M
Calculate the concentration of each ion: 0.18M K2CO3
0.18M, 0.36M, 0.54M
Calculate the concentration of each ion: 5.0 x 10-5 M Ag2CrO4
5.0 x 10-5, 1.0 x 10-4, 5.0 x 10-5
Calculate the concentration of each ion: 0.25M Na3PO4
0.25M, 0.75M, 0.25M
Calculate the concentration of each ion: 0.33M Cr2(SO4)3
0.33M, 0.66M, 0.99M
Calculate the concentration of each ion: 0.30M NaBr mixed with an equal volume of 0.50M CuBr2
Na=0.15M, Cu=0.25M, Br=0.65M
Calculate the concentration of each ion: 140.0mL of 0.36M CaCl2 mixed with 60.0mL of 0.22M Ca(NO3)2
Cl=0.50M, NO3=0.13M, Ca=0.32M
Calculate the volume required to prepare the diluted solution: Given 12M HNO3; need 250mL of 0.20M HNO3
0.0042L