Question
In: Chemistry
You dissolve 3.25 g of sodium oxalate (Na2C2O4) in sufficient water to produce a final solution...
You dissolve 3.25 g of sodium oxalate (Na2C2O4) in sufficient water to produce a final solution volume of 100.0 mL. Assuming all of the solid dissolves, calculate the solution pH.
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
1. You dissolve 5.00 g sodium hydrogen oxalate (NaHC2O4 ) in suffircient water to produce a...
1. You dissolve 5.00 g sodium hydrogen oxalate (NaHC2O4 ) in
suffircient water to produce a final solution volume of 100.0 mL.
Assuming all of the solid dissolves, calculate the pH of this
solution.
2. You dissolve 5.00 g of sodium oxalate (Na2C2O4) in sufficient
water to produce a final solution volume of 100.0 mL. Assuming all
of the solid dissolves, calculate the solution pH of this
solution.
3. You dissolve 5.00 g of sodium hydrogen oxalate and 5.00 g...
1. You dissolve 5.00 g sodium hydrogen oxalate (NaHC2O4 ) in suffircient water to produce a...
1. You dissolve 5.00 g sodium hydrogen oxalate (NaHC2O4 ) in
suffircient water to produce a final solution volume of 100.0 mL.
Assuming all of the solid dissolves, calculate the pH of this
solution.
2. You dissolve 5.00 g of sodium oxalate (Na2C2O4) in sufficient
water to produce a final solution volume of 100.0 mL. Assuming all
of the solid dissolves, calculate the solution pH of this
solution.
3. You dissolve 5.00 g of sodium hydrogen oxalate and 5.00 g...
In a volumetric analysis experiment, a solution of sodium oxalate (Na2C2O4) in acidic solution is titrated...
In a volumetric analysis experiment, a solution of sodium
oxalate (Na2C2O4) in acidic solution is titrated with a solution of
potassium permanganate (KMnO4) according to the following balanced
chemical equation:
2KMnO4(aq) + 8H2SO4(aq) + 5Na2C2O4(aq) →
2MnSO4(aq) + 8H2O(l) + 10CO2(g) +
5Na2SO4(aq) + K2SO4(aq)
What volume of 0.0393 M KMnO4 is required to titrate 0.142
g of Na2C2O4 dissolved in 30.0 mL of solution? PICK ONE.
A
27.0 mL
B
10.8 mL
C
30.0 mL
D
1.45 mL
E...
What is the pH of a 0.39 M solution of sodium oxalate, Na2C2O4? Acid ionization constants...
What is the pH of a 0.39 M solution of sodium oxalate,
Na2C2O4? Acid ionization constants
for oxalic acid are Ka1 = 5.6 x 10-2
and Ka2= 5.4 x 10-5.
A 25.00 mL solution containing 0.3000 M Na2C2O4 (sodium oxalate) was titrated with 0.1500 M Ca(NO3)2...
A 25.00 mL solution containing 0.3000 M Na2C2O4 (sodium oxalate)
was titrated with 0.1500 M Ca(NO3)2 to precipitate calcium oxalate:
Use Excel to draw a graph of pCa vs. VCa from 0 to 75 mL, using a
suitable resolution to show a sharp endpoint. Label the axes and
show where the end point lies.
A 6M H2SO4 solution will be used in preparing the sodium oxalate solution for titration in...
A 6M H2SO4 solution will be used in
preparing the sodium oxalate solution for titration in this
experiment.
a) Using your 100 mL graduated cylinder (and a piece of parafilm to
cover the mouth of the graduated cylider),
briefly explain, and show your calculations, how you will prepare
200 mL of 1 M H2SO4 for this purpose. (1
pt.)
b) What is the role of H2SO4 in the RedOx
reaction? (0.5 pt.)
If 2.99 g of sodium peroxide (Na2O2) react with water to produce sodium hydroxide and oxygen,...
If 2.99 g of sodium peroxide (Na2O2) react
with water to produce sodium hydroxide and oxygen, how many liters
of oxygen will be produced at 30.4 °C and 734 torr?
2 Na2O2(s) + 2
H2O(l) → 4 NaOH(aq) +
O2(g)
A.) what is the normality of Na2C2O4 solution if you use 1.14g of Na2C2O4 to prepare...
A.) what is the normality of Na2C2O4 solution if you use 1.14g
of Na2C2O4 to prepare 100.00 mL of solution?
B.) what is the normality of the stock KMnO4 solution if it took
31.20 mL of the KMnO4 solution to titrate a 20.00 mL sample of the
oxalate solution prepared in part a?
A solution is made by dissolving 10.0 g of sodium chloride in 110.5 g of water...
A solution is made by dissolving 10.0 g of sodium chloride in
110.5 g of water at 25oC. The density of the solution is 1.021
g/mL
1.What is the osmotic pressure of this solution?
2.What is the boiling point of this solution?
3.What is the freezing point of this solution?
We dissolve 4.44 g of an unknown acid, HA, in enough water to produce 25.0 mL...
We dissolve 4.44 g of an unknown acid, HA, in enough water to
produce 25.0 mL of solution. The pH of this solution of HA(aq) is
1.44. We titrate this solution with a 0.250 M solution of NaOH. It
takes 38.8 mL of the NaOH solution to reach the equivalence point.
The temperature is 25oC.
(a) What is the molar mass of HA?
(b) What is the pKa value of HA(aq)?
(c) What is the pH at the equivalence point?...
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