1.00 g mixture of Na2CO3and K2CO3was titrated with HCl. The
analysis shows that there are 8.00x10-3moles...
1.00 g mixture of Na2CO3and K2CO3was titrated with HCl. The
analysis shows that there are 8.00x10-3moles of CO3-2 ions.
Calculate the w/w% Na2CO3in the mixture.
The dibasic compound B (pKb1 = 4.00, pKb2 = 8.00) was titrated
with 1.00 M HCl. The initial solution of B was 0.100 M and had a
volume of 100.0 mL. Find the pH at the following volumes of acid
added and make a graph of pH versus Va; Va=0, 1, 5, 9, 10, 11, 15,
19, 20, and 22mL.
A gas mixture for use in some lasers contains 5.00 % by weight
HCl, 1.00 % H2, and 94 % Ne. The mixture is sold in cylinders that
have a volume of 49.0 L and a pressure of 13300 kPa at 21.0 ∘C
What is the partial pressure (in kilopascals) of each gas in the
mixture?
a mixture of 73.0 g NH3 and 73.0 g HCl are made to
react at stp according to the equation
NH3 + HCl --> NH4Cl
What is the volume of gas remaining and what gas is it?
Kw = 1.00 x 10-14
A 20.0 mL sample of 0.200M HCl solution is titrated
with 0.200M NaOH solution. Calculate the pH of the
solution after the following volumes of the base have been added.
Please show all work and explain. Thank you :)
a) 13.0 mL of NaOH
b) 28.0 mL of NaOH
A 4.10 −g sample of a mixture of CaO and BaO is placed in a
1.00-L vessel containing CO2 gas at a pressure of 735 torr and a
temperature of 26 ∘C. The CO2 reacts with the CaO and BaO, forming
CaCO3 and BaCO3. When the reaction is complete, the pressure of the
remaining CO2 is 155 torr .
Calculate the number of moles of CO2 that have reacted.
Calculate the mass percentage of CaO in the mixture.
An aqueous solution containing 1.00 g of oxobutanedioc acid (FM
132.07) per 100 mL was titrated with 0.09432 M NaOH.
Calculate the pH at th following volumes of added base:
0.5Ve1, Ve1, 1.5Ve2,
Ve2, 1.05Ve2
Sketch the titration curve, using the values calculated
above.
Which equivalence point would be best to use in this titration
(which one is not blurred)?
Ka1 = 2.56
Ka2 = 4.37
Ve1 = equivalence point 1
Ve2 = equivalence point 2
Mass data for reaction of NaHCO3-Na2CO3 mixture with HCL
Mass of crucible and cover (g)
28.8258
Mass of crucible, cover and mixture (g)
29.4948
Mass of crucible, cover and residue after reaction with HCL
(g)
1st weighing...
29.4454
2nd weighing...
29.4455
Calculation of percent NaHCO3 and Na2CO3 in an unknown mixture.
( I need help filling out this chart)
mass of unkown mixture used (g)
mass of NaCl formed (g)
Mass of NaHCO3 in unkown mixture (g)
Mass of Na2CO3...
A solution of 100.0 mL of 1.00 M malonic acid (H2A) was titrated
with 1.00 M NaOH. K1 = 1.49 x 10-2, K2 = 2.03 x 10-6. What is the
pH after 50.00 mL of NaOH has been added?
You have available 1.00 L volumes of the three following
solutions: 1.00 M HCl, 1.00 M NaOH and 1.00 M NaH2PO4. You wish to
prepare 500.0 mL of a buffer solution that maintains a pH of 2.50.
Indicate which two of these three solutions you would use to
produce this buffer, and calculate the volume of each of these two
solution you would need to mix to get the desired volume and pH
value for the buffer.
1.The total pressure of a mixture of O2(g) and H2(g) is 1.95
atm. The mixture is ignited and the resulting water is removed. The
remaining mixture is pure H2(g) and exerts a pressure of 0.210atm
when measured at the same temperature and volume as the original
mixture. What were the mole fractions of O2(g) and H2(g) in the
original mixture?