The end point of a titration was reached after 26.8 mL of 0.4 M disodium EDTA titrant was dispensed into a solution cont...
The end point of a titration was reached after 26.8 mL of 0.4 M disodium EDTA titrant was dispensed into a solution containing the zinc ion. Calculate the moles of disodium EDTA used.
Homework Answers
26 mL of 0.4 M disodium EDTA means that molarity of solution is 0.4 moles per litre/1000 mL
Add Answer to:
The end point of a titration was reached after 26.8 mL of 0.4 M disodium EDTA titrant was dispensed into a solution cont...
The end point of a titration was reached after 21.3 mL of 0.3 M disodium EDTA...
The end point of a titration was reached after 21.3 mL of 0.3 M disodium EDTA titrant was dispensed into a solution containing the zinc ion. Calculate the moles of disodium EDTA used.
The end point of the Zn2+−EDTA titration was observed after 21.50 mL of 0.0500 M EDTA solution was dispensed. Determine...
The end point of the Zn2+−EDTA titration was observed after 21.50 mL of 0.0500 M EDTA solution was dispensed. Determine the number of moles of zinc ion present in the sample. number of moles of zinc ion =
A titration was performed to standardize an EDTA solution. a) A 25.00 mL aliquot of a...
A titration was performed to standardize an EDTA solution. a) A 25.00 mL aliquot of a standard solution containing 0.01500 M Ca2+ required 42.87 mL of EDTA to reach the endpoint. The molarity of the EDTA solution is: ________ M b) That same EDTA solution was then used to titrate an unknown hard water sample. A 40.00 mL aliquot of unknown hard water required 34.21 mL of EDTA solution to reach a distinct endpoint. The concentration of Ca2+ ions (assuming...
3. Calculate in the titrant. 4. Another 1,00 mL of the NaOH solution is added after...
3. Calculate in the titrant. 4. Another 1,00 mL of the NaOH solution is added after the equivalence point. Calculate e reaction mixture. in the 5. Suppose 10.00 mL of water was added to the HCl solution before the titration was begun. How would your answers to questions 1-3 change? EXPERIMENT 10 Name QUANTITATIVE ANALYIS III STANDARDIZATION OF A STRONG BASE SOLUTION PRE-LAB EXERCISES Titration of 5.00 mL of a solution labeled 0.237 6 M HCl requires addition of 40.02...
The end point in a titration of a 76 mL sample of aqueous HCI was reached...
The end point in a titration of a 76 mL sample of aqueous HCI was reached by the addition of 63 mL of 0.23 M NaOH titrant. The reaction proceeds by the following equation. HCl(aq) + NaOH(aq) - NaCl(aq) + H2O(1) What is the molar concentration of HCI? Report your answer with two significant figures.
Titration of 5.00 mL of a solution labeled 0.237 6 M HCI requires addition of 40.02...
Titration of 5.00 mL of a solution labeled 0.237 6 M HCI requires addition of 40.02 mL of an NaOH solution to reach the equivalence point. 1. How many moles of HaO were used in the titration? 2. At the equivalence point, how many moles of OH had been added? 3. Calculate c in the titrant. OH in the OH 4. Another 1.00 mL of the NaOH solution is added after the equivalence point. Calculate c reaction mixture.
In a titration experiment, 11.4 mL of an aqueous HCl solution was titrated with 0.4 M...
In a titration experiment, 11.4 mL of an aqueous HCl solution was titrated with 0.4 M NaOH solution. The equivalence point in the titration was reached when 13.0 mL of the NaOH solution was added. What is the molarity of the HCl solution?
Problem 1: Consider titration of 24.0 mL of 0.0800 M Ga(NO3)3 with 0.0400 M EDTA at...
Problem 1: Consider titration of 24.0 mL of 0.0800 M Ga(NO3)3 with 0.0400 M EDTA at pH 4.00. (a) Calculate pGa+ (to the 2nd digit after the decimal point) upon addition of 10.00 mL of the EDTA solution. Log Ki= 20.30. (b) What is the pGa at the equivalence point of this titration? (C) What is the pGa upon addition of 50.00 mL of the EDTA solution?
In a titration experiment, 11.7 mL of an aqueous H2SO4 solution was titrated with 0.4 M...
In a titration experiment, 11.7 mL of an aqueous H2SO4 solution was titrated with 0.4 M NaOH solution. The equivalence point in the titration was reached when 10.7 mL of the NaOH solution was added. What is the molarity of the H2SO4 solution? H2SO4 molarity
1. What is the amount in grams of EDTA you will need to measure out to...
1. What is the amount in grams of EDTA you will need to measure out to prepare a 250 mL 0.01 M EDTA solution ? The molar mass of EDTA is 374.27 g/mol. 2. Titration Data from three water samples Water Volume of 0.01 Water Drops of MEDTA Moles Ca2+ sample indicator used to of concentration volume Calmagite reach Ca2+ in water (M) end point source 50 mL4 2 ml USFISA drinking water fountain USF BSF drinking water fountain 50...
3. Calculate in the titrant. 4. Another 1,00 mL of the NaOH solution is added after the equivalence point. Calculate e reaction mixture. in the 5. Suppose 10.00 mL of water was added to the HCl solution before the titration was begun. How would your answers to questions 1-3 change? EXPERIMENT 10 Name QUANTITATIVE ANALYIS III STANDARDIZATION OF A STRONG BASE SOLUTION PRE-LAB EXERCISES Titration of 5.00 mL of a solution labeled 0.237 6 M HCl requires addition of 40.02...
The end point in a titration of a 76 mL sample of aqueous HCI was reached by the addition of 63 mL of 0.23 M NaOH titrant. The reaction proceeds by the following equation. HCl(aq) + NaOH(aq) - NaCl(aq) + H2O(1) What is the molar concentration of HCI? Report your answer with two significant figures.
Titration of 5.00 mL of a solution labeled 0.237 6 M HCI requires addition of 40.02 mL of an NaOH solution to reach the equivalence point. 1. How many moles of HaO were used in the titration? 2. At the equivalence point, how many moles of OH had been added? 3. Calculate c in the titrant. OH in the OH 4. Another 1.00 mL of the NaOH solution is added after the equivalence point. Calculate c reaction mixture.
Problem 1: Consider titration of 24.0 mL of 0.0800 M Ga(NO3)3 with 0.0400 M EDTA at pH 4.00. (a) Calculate pGa+ (to the 2nd digit after the decimal point) upon addition of 10.00 mL of the EDTA solution. Log Ki= 20.30. (b) What is the pGa at the equivalence point of this titration? (C) What is the pGa upon addition of 50.00 mL of the EDTA solution?
1. What is the amount in grams of EDTA you will need to measure out to prepare a 250 mL 0.01 M EDTA solution ? The molar mass of EDTA is 374.27 g/mol. 2. Titration Data from three water samples Water Volume of 0.01 Water Drops of MEDTA Moles Ca2+ sample indicator used to of concentration volume Calmagite reach Ca2+ in water (M) end point source 50 mL4 2 ml USFISA drinking water fountain USF BSF drinking water fountain 50...
Most questions answered within 3 hours.
-
This picture is a visual representation of helium. Write the
chemical formula for helium.
asked 4 seconds ago -
1. Sample Mean:
mens- 27.91
women - 31.57
2. Standard Deviation
men- 0.664
women- 1.167
Sample...
asked 10 minutes ago -
Needs Help with Java Programming language!
Lights Camera
Action Purpose: To learn the basics of linked...
asked 8 minutes ago -
Please answer my questions:
True or False and Explain
5)In a perfectly competitive market, if price...
asked 13 minutes ago -
Suppose the interest on a foreign government bonds is 7.5%, and
the current exchange rate is...
asked 14 minutes ago -
Explain why it is important to know common Windows processes
when conducting a forensic investigation
asked 19 minutes ago -
How do child protective services help to reduce the
vulnerability of minors to human trafficking?
asked 27 minutes ago -
Which of the following is correct?
a. ATC = AVC/Q
b. ATC = AFC/Q
c. ATC...
asked 27 minutes ago -
The height of a Harrier airplane above the ground is given by h
= 4.00t 3...
asked 36 minutes ago -
Subject Conflict resolution :
1-Describe the basic model for engaging someone in a
collaborative discussion in...
asked 36 minutes ago -
Using the four models of CSR, and given your own personal
values, what type of firm...
asked 40 minutes ago -
A 10 kg mass slides along a frictionless plane inclined at 38
degrees to the horizontal....
asked 44 minutes ago