Please show work.... 1. A 10.00 mL choride sample required 33.65 mL of .01251 M AgNO3...
Please show work....
1. A 10.00 mL choride sample required 33.65 mL of .01251 M AgNO3 to reach the end point.
a) How many moles of Cl- were present in the sample?
b) What was the molarity of the Cl- sample?
Homework Answers
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Please show work....
1. A 10.00 mL choride sample required 33.65 mL of .01251 M AgNO3...
How many grams of AgNO3 are required to make 770.0 mL of a 0.15 M solution?...
How
many grams of AgNO3 are required to make 770.0 mL of a 0.15 M
solution?
How many grams of AgNO3 are required to make 770.0 mL of a 0.15 M solution? The molar mass of silver nitrate is 169.9 g/mol. One approach is to solve the molarity relationship (M- n/N) for moles. o a 19.6g b. 6.82 g O5.10 g o d. 1.95 g O e. None of the above
please show all work. thank you A 10. equivalence point. L sample of vinegar, an aqueous solution of acetic acid (HC2H02), is titrated with 0.5003 M NaOH, and 15.00 mL is required to reach the a....
please show all work. thank you
A 10. equivalence point. L sample of vinegar, an aqueous solution of acetic acid (HC2H02), is titrated with 0.5003 M NaOH, and 15.00 mL is required to reach the a. What is the molarity of the acetic acid? b. If the density of the vinegar is 1.006 g/cm3, what is the mass percent of acetic acid in the vinegar?
A 10. equivalence point. L sample of vinegar, an aqueous solution of acetic acid (HC2H02),...
2) A solution of I2 was standardized with ascorbic acid. The titration of a 10.00 mL...
2) A solution of I2 was standardized with ascorbic acid. The titration of a 10.00 mL aliquot of a stock solution made by dissolving 0.1050 g sample of pure ascorbic acid to a final volume of 100.00 mL required 25.32 mL of I2 to reach the starch end point a. What is the molarity of the iodine solution? b. How many mg ascorbic acid is required to react with 1.00 mL iodine solution?
10.0 mL of unknown CL- solution requires 22.0 mL of 0.050 M AgNO3 to reach the...
10.0 mL of unknown CL- solution requires 22.0 mL of 0.050 M AgNO3 to reach the end point. What is the concentration of Cl- in the unknown? If the solution was prepared by dissolving 1.00 g of solid in 100 mL, what is the weight % CL- in the solid? Ag+ + CL- -------> AgCl
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...
please show work? Question 33 (8 points) A 28.7 mL sample of KOH required 31.3 mL...
please show work?
Question 33 (8 points) A 28.7 mL sample of KOH required 31.3 mL of 0.118 M H2SO3 to neutralize it. How many grams of KOH were in the original sample? 2KOH + H2SO3 ----> K2503 + 2H20 Please leave a space between the number and unit in your answer.
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 +...
a. If a titration of a sample of HCl dissolved in water required 33.56 mL of...
a. If a titration of a sample of HCl dissolved in water required 33.56 mL of 0.0358 M NaOH, how many moles of HCl were in the sample? b. What is the molarity of a solution that results from dissolving 0.895 g of Na2CO3 in 50 mL of water, then diluting the mixture by a factor of 1:25?
2. A 10.00 mL sample of aqueous H2SO, requires 20.00 mL of 0.201 M NaOH to...
2. A 10.00 mL sample of aqueous H2SO, requires 20.00 mL of 0.201 M NaOH to reach the endpoint. Calculate the molarity of H2SO4
2. A student performs a titration on a 5.00 mL sample of an HBr solution. She...
2. A student performs a titration on a 5.00 mL sample of an HBr solution. She uses 24.32 mL of a 0.459 M KOH solution to reach a phenolphthalein endpoint. (See Example 2, if necessary.) a. Write the balanced equation for the reaction. Remember to include the correct physical states for each reactant and product in your balanced equation. b. How many moles of KOH were used? C. How many moles of HBr were present? d. What is the molarity...
How
many grams of AgNO3 are required to make 770.0 mL of a 0.15 M
solution?
How many grams of AgNO3 are required to make 770.0 mL of a 0.15 M solution? The molar mass of silver nitrate is 169.9 g/mol. One approach is to solve the molarity relationship (M- n/N) for moles. o a 19.6g b. 6.82 g O5.10 g o d. 1.95 g O e. None of the above
please show all work. thank you
A 10. equivalence point. L sample of vinegar, an aqueous solution of acetic acid (HC2H02), is titrated with 0.5003 M NaOH, and 15.00 mL is required to reach the a. What is the molarity of the acetic acid? b. If the density of the vinegar is 1.006 g/cm3, what is the mass percent of acetic acid in the vinegar?
A 10. equivalence point. L sample of vinegar, an aqueous solution of acetic acid (HC2H02),...
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...
please show work?
Question 33 (8 points) A 28.7 mL sample of KOH required 31.3 mL of 0.118 M H2SO3 to neutralize it. How many grams of KOH were in the original sample? 2KOH + H2SO3 ----> K2503 + 2H20 Please leave a space between the number and unit in your answer.
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 +...
2. A 10.00 mL sample of aqueous H2SO, requires 20.00 mL of 0.201 M NaOH to reach the endpoint. Calculate the molarity of H2SO4
2. A student performs a titration on a 5.00 mL sample of an HBr solution. She uses 24.32 mL of a 0.459 M KOH solution to reach a phenolphthalein endpoint. (See Example 2, if necessary.) a. Write the balanced equation for the reaction. Remember to include the correct physical states for each reactant and product in your balanced equation. b. How many moles of KOH were used? C. How many moles of HBr were present? d. What is the molarity...
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