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A 25.0 ml sample of hcl was titrated to the endpoint with 15.0 ml of 2.0 normality naoh what was the normality of th hcl what was its molarity?
Lissaliss
The HCL concentration is 1.2M or 1.2N
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A 25.00 mL sample of HBr is titrated with 0.150 M standardized sodium hydoxide solution the endpoint was reached when 18.80 mL of titrant had been added calculate the molar concentration of the HBr?
(25.00ml HBr)( Molarity ) = ( 18.80ml NaOH )( 0.150 M ) Molar concetration of HBr = 0.108 M
A corrosion technologist pipetted a 100 ml hard water sample and titrated it with 37.64 ml of 0.01 m edta solution for a total hardness endpoint and 29.32 ml of 0.01 m edta solution for a calcium?
3.00 M
Would the reported molarity of the vinegar sample be affected by an error in weighing?
Yes, you could possibly have errors in your data about the molarity of a vinegar sample during a titration experiment if there was an error made during weighing.
What is the endpoint of a titration?
during a titration when a titrant completely furnished the sample then this is the end point of titration.
A 3.0-milliliter sample of hno3 solution is exactly neutralized by 6.0 milliliters of 0.50 m koh what is the molarity of the hno3 sample?
1.0 Moles
A 25.00 mL sample of HBr is titrated with 0.150 M standardized sodium hydoxide solution the endpoint was reached when 18.80 mL of titrant had been added calculate the molar concentration of the HBr?
(25.00ml HBr)( Molarity ) = ( 18.80ml NaOH )( 0.150 M ) Molar concetration of HBr = 0.108 M
A corrosion technologist pipetted a 100 ml hard water sample and titrated it with 37.64 ml of 0.01 m edta solution for a total hardness endpoint and 29.32 ml of 0.01 m edta solution for a calcium?
3.00 M
What is the molarity of a 2.5 L sample that contains 15 moles of NaCl?
The molarity is 6.
Would the reported molarity of the vinegar sample be affected by an error in weighing?
Yes, you could possibly have errors in your data about the molarity of a vinegar sample during a titration experiment if there was an error made during weighing.
A sample of 76g of NaCl is dissolved to make 1L of solution. what is the molarity of the solution?
1.3g
What is the endpoint of a titration?
during a titration when a titrant completely furnished the sample then this is the end point of titration.
A 3.0-milliliter sample of hno3 solution is exactly neutralized by 6.0 milliliters of 0.50 m koh what is the molarity of the hno3 sample?
1.0 Moles
How do you prepare analyte?
The substance to be analysed normally of unknown quantity is called as analyte. it is called as sample. In titration of analytes normally we take it according to the Normality of the titrant taken to find the quantity of analyte. Sample Size = Titer Value*Normality*Molecularr(or)equivalent weight/ purity/10. This formula is expressed in terms of %.
Why is a titration performed?
To find the unknown concentration of a sample by using a reagent with a known concentration. ( IE; molarity )
What is the concentration of a nitric acid solution if a 10.00 mL sample of the acid requires 31.25 mL of 0.135 M KOH for neutralization?
In an acid-base titration problem, the formula to use is: MaVa = MbVb, where the molarity of the acid times its volume equals the molarity of the base times its volume.Here, we have:Ma(10.00mL) = (0.135M)(31.25mL)Solving for Ma = 4.22M.mL / 10.00mL = 0.422M(Note: This is only valid for monoprotic acid with monoprotic bases only, as in this case. If it were titrated with 0.135M carbonate (CO32-) the findings need to be doubled.)
A 20.0 mL sample of CuSO4 was evaporated to dryness leaving 0.967g of residue What was the molarity of the original solution?
Molarity = moles of solute(CuSO4)/volume of solution(Liters) 0.967 grams CuSO4 (1 mole CuSO4/159.62 grams) = 0.00606 moles CuSO4 Molarity = 0.00606 moles/0.020 liters = 0.303 Molarity
A 25 ml sample of 723 m hclo4 is titrated with a 273 m koh solution the h3o concentration after 66.2 ml of koh is?
1.00x10^-7
