Questions LLC
Login
or
Sign Up
Ask a New Question
Chemistry
Stoichiometry
Molarity
What is the molarity of the solution containing 6.245g of oxalic acid, H2C2O4 in 750mL
1 answer
mols H2C2O4 = grams/molar mass, then
M = mols/L
You can
ask a new question
or
answer this question
.
Similar Questions
What is the mole of oxalic acid?
Equation:H2C2O4 + 2NaOH---> Na2C2O4 + 2H2O *Moles of oxalic acid dihydrate is 0.032 mole. *
Top answer:
To determine the number of moles of oxalic acid, we can use the provided information about the moles
Read more.
What is the mole of oxalic acid?
Equation:H2C2O4 + 2NaOH---> Na2C2O4 + 2H2O *Moles of oxalic acid dihydrate is 0.032 mole. *
Top answer:
NaOH
Read more.
20.5 mL of oxalic acid,H2C2O4 were titrated with 0.800 M solution of lithium hydroxide. It took 40.0 mL of the base to reach the
Top answer:
H2C2O4 + 2LiOH ==> LiC2O4 + 2H2O moles oxalic acid = M x L. moles LiOH = 2x moles oxalic acid (from
Read more.
1. A sample of oxalic acid (H2C2O4, with two acidic protons), of volume 46.56 mL was titrated to the stoichiometric point with
Top answer:
To find the molarity of oxalic acid and the mass of oxalic acid in the given sample, we can use the
Read more.
100mL of oxalic acid (H2C2O4) requires 35mL of 0.04 M KMnO4 to titrate it to the endpoint. calculate the molarity of the oxalic
Top answer:
5H2C2O4 + 2KMnO4 + 3H2SO4 ==> 10CO2 + 8H2O + 2MnSO4 + K2SO4 millimoles KMnO4 = mL x M = 35 mL x 0.04
Read more.
100mL of oxalic acid (H2C2O4) requires 35mL of 0.04M KMnO4 to titrate it to the endpoint. calculate the molarity of the oxalic
Top answer:
0.035
Read more.
A sample of oxalic acid (H2C2O4, with two acidic protons), of volume 37.09 mL was titrated to the stoichiometric point with
Top answer:
show me your thinking on this.
Read more.
25.00 mL of a solution of oxalic acid are titrated with 0.2586 m NaOH (aq). The stoichiometric eend point is reached when 43.42
Top answer:
And I don't think 0.044 is it. I would call your attention to the 0.2586m NaOH. If that should be
Read more.
A solution is prepared by dissolving 0.5842g of oxalic acid (H2C2O4) in enough water to make 100.0ml of solution. A 10.00ml
Top answer:
The final answer is 10000 ????
Read more.
How do you find the Ka1 and Ka2 of oxalic acid when it is in a solution that is 1.05 M H2C2O4 and has a pH of 0.67. [C2O4^2-] =
Top answer:
You know the concentration of the chromate ion (above), then let the concentration of the bichromate
Read more.
Related Questions
a 69.3g sample of oxalic ac acid, H2C2O4, was dissolved in 1.000L of solution. How would yo prepare 1.00L of 0.150M H2C2O4 from
H2C2O4.2H2O(s) is primary standard substance. 2.3688g of oxalic acid hydrate were completely neutralized by 42.56ml of NaOH
A 1.575 g sample of ethanedioic acid crystals, H2C2O4. xH20 was dissolved in water and made up to 250cm^3 . One mole of the acid
A 0.5537-g sample containing oxalic acid required 21.62 mL of 0.09377 M NaOH for titration. If the reaction is H2C2O4 + 2NaOH
Calculate the molarity of a sodium hydroxide solution if 10.42 mL of this solution are needed to neutralize 25.00 mL of 0.2043 M
How many Kilograms of water must be added to 5.0 grams of oxalic acid (H2C2O4) to prepare a 0.40 Molality?
a 5.55g sample of a weak acid with ka=1.3*10^-4 was combined with 5.00ml of 6.00 M NAOH and the resulting solution was diluted
Oxalic acid, found in the leaves of rhubarb and other plants, is a diprotic acid.
H2C2O4 + H2O ↔ H3O+ + HC2O4- Ka1= ? HC2O4- +
What mass of oxalic acid dihydrate , H2C2O4•2H2O, is required to prepare 220.0 ml of a 1.28 M solution of oxalic acid ?
prepare M/20 solution of oxalic acid. Find out the molarity and strength in gram per litre of the given solution of potassium