Question

If the standard calcium carbonate solution is 100ppm and 25ml of solution is used for the...

If the standard calcium carbonate solution is 100ppm and 25ml of solution is used for the standardization, calculate the approximate volume of 2 mM EDTA solution needed to reach the end point of the titration.

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The density of the sample is 0.9977 g/mL, and the molar mass of calcium carbonate is...
The density of the sample is 0.9977 g/mL, and the molar mass of calcium carbonate is 100.0 g/mol. Calculate the mass of calcium carbonate present in a 50.00 mL sample of an aqueous calcium carbonate standard, assuming the standard is known to have a hardness of 75.0 ppm. If this wsa titrated with a 0.00501 M EDTA, what volume of EDTA solution would be needed to reach the endpoint? (using the given density of this problem is throwing me off...
25ml of a sample of tap water and 25ml sample duplicate were taken and titrated with...
25ml of a sample of tap water and 25ml sample duplicate were taken and titrated with an EDTA solution. 5.1ml and 5.2ml of titrant was used respectively. Determine the concentration of the hardness of the sample and duplicate in mg of calcium carbonate/L, the mean, standard deviation, and the %RSD. If the specification for %RSD < 2.9% and the relative error < 5%, what can be said about the precision of analysis.
An artificial Dolomite containing calcium carbonate and magnesium carbonate weighing 1.0200g was reacted with 50.0mL of...
An artificial Dolomite containing calcium carbonate and magnesium carbonate weighing 1.0200g was reacted with 50.0mL of 0.920M hydrochloric acid to produce a solution. The excess hydrochloric acid in the solution required 38.1mL of.0 630M sodium hydroxide to complete the titration. Calculate the percentage of each component in the mixture.
You have been tasked with determining the concentration of Ca2+ in an unknown solution of calcium...
You have been tasked with determining the concentration of Ca2+ in an unknown solution of calcium carbonate (CaCO3). You titrate 50.0 ml of the unknown solution with 0.0250 M EDTA. It requires 16.85 ml of EDTA to reach the equivalence point. Determine [Ca2+] of the unknown solution, in ppm. Recall that ppm (parts per million) is equal to mg/L. 2. If a sample of tap water contains 400 ppm of Ca2+ and 80 ppm of Mg2+, what is the hardness...
The amount of calcium in physiological fluids can be determined by a complexometric titration with EDTA....
The amount of calcium in physiological fluids can be determined by a complexometric titration with EDTA. In one such analysis a 0.100-mL sample of a blood serum was made basic by adding 2 drops of NaOH and titrated with 0.00119 M EDTA, requiring 0.268 mL to reach the end point. Report the concentration of calcium in the sample as milligrams Ca per 100 mL.
Calculate the volume of a standard solution needed to reach the end point. -Calculate the molarity...
Calculate the volume of a standard solution needed to reach the end point. -Calculate the molarity of 25.0mL of an HCl solution titrated with 0.16M NaOH solution. The end Point was reached when 24.3mL of the standard solution was added. -Calculate the molarity of a standard solution of KOH if 18.0mL of the solution was needed to titrate 0.919g of KHP.
1. A 0.0352 g sample of pure calcium carbonate (100.09 g/mol) was dissolved in acid and...
1. A 0.0352 g sample of pure calcium carbonate (100.09 g/mol) was dissolved in acid and titrated to its endpoint with newly made EDTA titrant (~0.010 M) according to the procedure given below. The starting burette volume was 0.10 mL. The ending burette volume was 35.52 mL. Calculate the exact concentration of the EDTA titrant. Show all work.
A titration of Cu2+ with EDTA (abbreviated Y4-) is performed using an Erio-Black T indicator. The...
A titration of Cu2+ with EDTA (abbreviated Y4-) is performed using an Erio-Black T indicator. The titration has an error of +0.10% (if the titration should have used 100 mL to reach the equivalence point, it actually used 100.1 mL because of the end point error. Assume the titration involved 100 mL of 0.01 M Cu2+ and a 0.02 M EDTA titrant. The reaction is Cu2+ + Y4- → CuY2- K = 2 x 109 a) What volume of EDTA...
A 0.4505 g sample of CaCO3 was dissolved in the HCl and the resulting solution diluted...
A 0.4505 g sample of CaCO3 was dissolved in the HCl and the resulting solution diluted to 25.00 mL in a volumetric flask. A 25.00 mL aliquot of the solution required 29.25 mL of EDTA solution for titration to the Eriochrom Black T end point. a. How many moles of CaCO3 were present in the solid sample? b. What is the molar concentration of Ca^2+ are contained in a 250.00 mL aliquot of the CaCl2 solution? c. How many moles...
The reaction between the hydrochloric acid and the calcium carbonate is: 2 HCl (aq) + CaCO3...
The reaction between the hydrochloric acid and the calcium carbonate is: 2 HCl (aq) + CaCO3 (s) ---> CaCl2 (aq) + H2O (l) + CO2 (g) About 90 mL of water and 10.00 mL of 0.5023 M Hydrochloric acid solution was added to a 1.028 g paper sample. Following our procedure the mixture was stirred and then heated just to a boiling to expel the carbon dioxide. Titration of the excess HCl remaining in the mixture required 16.41 mL (corrected...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT