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Post-lab Questions 1. Ca n you titrate a solution of unknown concentration with another solution of...
7. You are given a solution of unknown concentration of HCI. (8 Points) You are asked...
7. You are given a solution of unknown concentration of HCI. (8 Points) You are asked to determine its concentration by titration. You made up a 0.25 moles/Liter solution of NaOH. You filled the burette with NaOH up to the mark. You measured 10 mL of the HCl solution into an Ehrlenmeyer flask and added 1 drop of the phenol- phthalein indicator You titrated the HCl in the Ehrlenmeyer flask with NaOH from the burette 3 times. Your observations were:...
Questions 3, 4, & 5 pls (3) You will titrate a solution of an unknown acid...
Questions 3, 4, & 5 pls
(3) You will titrate a solution of an unknown acid (HX(aq)) by adding NaOH(aq). Suppose that 25 mL of 0.5 M NaOH(aq) is needed to reach the equivalence point. How many moles of HX were present initially? Show the calculation. (4) You will titrate acid solutions by adding 0.2-0.3-mL or 2-3-mL portions of NaOH(aq). When should you add the smaller volume? (5) The concentration of an aqueous solution of NaOH cannot be accurately determined...
An aqueous solution of Ca(OH)2with a concentration of 0.161 M was used to titrate 25.00 mL...
An aqueous solution of Ca(OH)2with a concentration of
0.161 M was used to titrate 25.00 mL of aqueous HCl. 18.63
mL of the Ca(OH)2was required to reach the endpoint of
the titration.
Part 1 (1 point) How many moles of base were required to react completely with the acid in this reaction? x 10 mol Ca(OH)2 -- Part 2 (1 point) How many moles of HCl were present in the original 25.00 mL of acid? x 10 mol HCl +...
An aqueous solution of Ca(OH)2with a concentration of 0.143 M was used to titrate 25.00 mL...
An aqueous solution of Ca(OH)2with a concentration of
0.143 M was used to titrate 25.00 mL of aqueous HCl. 14.73
mL of the Ca(OH)2was required to reach the endpoint of
the titration.
How many moles of base were required to react completely with the
acid in this reaction?
How many moles of HCl were present in the original 25.00 mL of
acid?
What is the molarity of the original HCl solution?
04 Question (a points) aSee page 166 Watch the...
This is chemistry lab, Analysis of Unknown Base sample :Using Titation Curve to Deterime formula ...
this is chemistry lab, Analysis of Unknown Base sample :Using
Titation Curve to Deterime formula Weight and Pk
Questions If we the point? had used an indicator instead of a titration curve, we would have found the endpoint of titration. What is the difference between and indicator endpoint and the equivalence 1. If the concentration of the HCI titrant was wrong during your experiment, which of your values would also be incorrect, the molar mass or the pK, or both?...
The titration of 23.30 mL of HCl solution of unknown concentration requires 13.00 mL of a...
The titration of 23.30 mL of HCl solution of unknown concentration requires 13.00 mL of a 0.200 M NaOH solution to reach the equivalence point. What is the concentration of the unknown HCl solution in M? Express your answer in moles per liter to three significant figures. M(HCl)M(HCl) = _____________
The titration of 29.40 mL of HCl solution of unknown concentration requires 12.82 mL of a...
The titration of 29.40 mL of HCl solution of unknown concentration requires 12.82 mL of a 0.150 M NaOH solution to reach the equivalence point. What is the concentration of the unknown HCl solution in M?
To determine the Ca^2+ concentration in water sample, a standard EDTA solution of 0.01988 M was...
To determine the Ca^2+ concentration in water sample, a standard EDTA solution of 0.01988 M was used to titrate 25 ml. of the sample solution with the presence of an ammonium buffer (pH 10). If 15.80 ml. of the standard EDTA was used to reach the end point, calculate the molar concentration and the ppm concentration of the unknown Ca^2+ (atomic weight of Ca = 40.08g/mole) solution The amount of 0.2915g of benzoic acid was dissolved in 100 ml. of...
You have titrated 30.00mL of an unknown Ca(OH)2(aq) solution to the second equivalence point with 34.93mL...
You have titrated 30.00mL of an unknown Ca(OH)2(aq) solution to the second equivalence point with 34.93mL of 0.417M HCl(aq). What is the concentration of the Ca(OH)2(aq) solution?
A 25.0 mL NaOH solution of unknown concentration was titrated with a 0.189 M HCl solution....
A 25.0 mL NaOH solution of unknown concentration was titrated with a 0.189 M HCl solution. 19.6 mL HCl was required to reach equivalence point. In a separate titration, a 10.0 mL H3PO4 solution was titrated with the same NaOH solution. This time, 34.9 mL NaOH was required to reach the equivalence point. What is the concentration of the H3PO4 solution?
7. You are given a solution of unknown concentration of HCI. (8 Points) You are asked to determine its concentration by titration. You made up a 0.25 moles/Liter solution of NaOH. You filled the burette with NaOH up to the mark. You measured 10 mL of the HCl solution into an Ehrlenmeyer flask and added 1 drop of the phenol- phthalein indicator You titrated the HCl in the Ehrlenmeyer flask with NaOH from the burette 3 times. Your observations were:...
Questions 3, 4, & 5 pls
(3) You will titrate a solution of an unknown acid (HX(aq)) by adding NaOH(aq). Suppose that 25 mL of 0.5 M NaOH(aq) is needed to reach the equivalence point. How many moles of HX were present initially? Show the calculation. (4) You will titrate acid solutions by adding 0.2-0.3-mL or 2-3-mL portions of NaOH(aq). When should you add the smaller volume? (5) The concentration of an aqueous solution of NaOH cannot be accurately determined...
An aqueous solution of Ca(OH)2with a concentration of
0.161 M was used to titrate 25.00 mL of aqueous HCl. 18.63
mL of the Ca(OH)2was required to reach the endpoint of
the titration.
Part 1 (1 point) How many moles of base were required to react completely with the acid in this reaction? x 10 mol Ca(OH)2 -- Part 2 (1 point) How many moles of HCl were present in the original 25.00 mL of acid? x 10 mol HCl +...
An aqueous solution of Ca(OH)2with a concentration of
0.143 M was used to titrate 25.00 mL of aqueous HCl. 14.73
mL of the Ca(OH)2was required to reach the endpoint of
the titration.
How many moles of base were required to react completely with the
acid in this reaction?
How many moles of HCl were present in the original 25.00 mL of
acid?
What is the molarity of the original HCl solution?
04 Question (a points) aSee page 166 Watch the...
this is chemistry lab, Analysis of Unknown Base sample :Using
Titation Curve to Deterime formula Weight and Pk
Questions If we the point? had used an indicator instead of a titration curve, we would have found the endpoint of titration. What is the difference between and indicator endpoint and the equivalence 1. If the concentration of the HCI titrant was wrong during your experiment, which of your values would also be incorrect, the molar mass or the pK, or both?...
To determine the Ca^2+ concentration in water sample, a standard EDTA solution of 0.01988 M was used to titrate 25 ml. of the sample solution with the presence of an ammonium buffer (pH 10). If 15.80 ml. of the standard EDTA was used to reach the end point, calculate the molar concentration and the ppm concentration of the unknown Ca^2+ (atomic weight of Ca = 40.08g/mole) solution The amount of 0.2915g of benzoic acid was dissolved in 100 ml. of...
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