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2. A student performs a titration on a 5.00 mL sample of an HBr solution. She...
1. A student performs a titration that requires 40.00 mL of 0.5000 M KOH to completely...
1. A student performs a titration that requires 40.00 mL of 0.5000 M KOH to completely react with 30.00 mL of a H3PO4 solution. What is the molarity of the H3PO4 solution, if the two compounds react according to this equation? (HINT: DO NOT use MiV=M2V2 to solve for the molarity of acid involved in a titration!) H3PO4 (aq)+ 3 KOH(aq) → K3PO4 (aq) + 3 H2O(1)
A titration of 25.00 mL of O.1550 M HCl solution with a solution of NaOH of...
A titration of 25.00 mL of O.1550 M HCl solution with a solution of NaOH of unknown molarity starts at a buret reading for NaOH of 0.33 mL The phenolphthalein indicator turns light pink the acid solution for over 30 seconds at a buret reading of 24.19 mL 2) What was the volume of HCl you started with? 3) How many moles of HCl were in the original solution? 4) Write the balanced chemical equation for the titration reaction. 5)...
answer (2) 2. Suppose that you used a known concentration (0.8442 M) of Ca(OH)2 to determine...
answer (2)
2. Suppose that you used a known concentration (0.8442 M) of Ca(OH)2 to determine the concentration of an unknown HBr solution. If it takes 12.88 mL of the Ca(OH)2 solution to titrate 15.00 mL of the unknown HBr solution, what is the molarity of the HBr? 1. A solid diprotic weak acid, H2A (molecular weight = 128.9 g/mol) is used to standardize a KOH solution. When 0.4228 g of the acid is dissolved in 40.0 mL of water...
A student is trying to determine the concentration of an acetic acid (HC2H302) solution. They place...
A student is trying to determine the concentration of an acetic acid (HC2H302) solution. They place 5.00 mL of it in a flask and titrate it with a 0.150 M NaOH solution. At the endpoint of the titration, they find that they have used 19.27 mL of the NaOH solution. Based on this information answer the following questions. a) How many moles of NaOH are used to reach the endpoint? moles NaOH b) How many moles of acetic acid were...
A student is trying to determine the concentration of an acetic acid (HC2H3O2) solution. They place...
A student is trying to determine the concentration of an acetic acid (HC2H3O2) solution. They place 5.00 mL of it in a flask and titrate it with a 0.150 M NaOH solution. At the endpoint of the titration, they find that they have used 19.27 mL of the NaOH solution. Based on this information answer the following questions. a) How many moles of NaOH are used to reach the endpoint? ____moles NaOH b) How many moles of acetic acid were...
QUESTION 19 A student is trying to determine the concentration of an acetic acid (HC31,0) solution....
QUESTION 19 A student is trying to determine the concentration of an acetic acid (HC31,0) solution. They place 5.00 mL of it in a flask and titrate it with a 0.150 M NaOH solution. At the endpoint of the titration they find that they have used 19.27 mL of the NaOH solution Based on this information answer the following questions. a) How many moles of NaOH are used to reach the endpoint? moles NaOH b) How many moles of acetic...
5.00 mL of a solution containing a monoprotic acid was placed in a 100-mL volumetric flask,...
5.00 mL of a solution containing a monoprotic acid was placed in a 100-mL volumetric flask, diluted to the mark with deionized water and mixed well. Then, 25.00 mL of this diluted acid solution was titrated with 0.08765 M NaOH. 9.23 mL of NaOH was required to reach the endpoint. a. What does the term monoprotic mean? b. Determine the molar ratio between the acid and NaOH. c. Calculate the moles of NaOH used in this titration. d. Calculate the...
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.
QUESTION 19 A student is trying to determine the concentration of an acetic acid (HC31,0) solution....
QUESTION 19 A student is trying to determine the concentration of an acetic acid (HC31,0) solution. They place 5.00 mL of it in a flask and titrate it with a 0.150 M NaOH solution. At the endpoint of the titration they find that they have used 19.27 mL of the NaOH solution Based on this information answer the following questions. a) How many moles of NaOH are used to reach the endpaint? moles NaOH b) How many moles of acetic...
In a titration, a student found that 42.6 mL of a KOH solution were required to...
In a titration, a student found that 42.6 mL of a KOH solution were required to neurtralize 28.9 mL of a 0.160 M sulfuric acid solution. Determine the molarity of the KOH solution. SHOW WORK. 2KOH(aq) + H2SO4(aq) ------> K2SO4(aq) + 2H2O(l)
1. A student performs a titration that requires 40.00 mL of 0.5000 M KOH to completely react with 30.00 mL of a H3PO4 solution. What is the molarity of the H3PO4 solution, if the two compounds react according to this equation? (HINT: DO NOT use MiV=M2V2 to solve for the molarity of acid involved in a titration!) H3PO4 (aq)+ 3 KOH(aq) → K3PO4 (aq) + 3 H2O(1)
answer (2)
2. Suppose that you used a known concentration (0.8442 M) of Ca(OH)2 to determine the concentration of an unknown HBr solution. If it takes 12.88 mL of the Ca(OH)2 solution to titrate 15.00 mL of the unknown HBr solution, what is the molarity of the HBr? 1. A solid diprotic weak acid, H2A (molecular weight = 128.9 g/mol) is used to standardize a KOH solution. When 0.4228 g of the acid is dissolved in 40.0 mL of water...
A student is trying to determine the concentration of an acetic acid (HC2H302) solution. They place 5.00 mL of it in a flask and titrate it with a 0.150 M NaOH solution. At the endpoint of the titration, they find that they have used 19.27 mL of the NaOH solution. Based on this information answer the following questions. a) How many moles of NaOH are used to reach the endpoint? moles NaOH b) How many moles of acetic acid were...
QUESTION 19 A student is trying to determine the concentration of an acetic acid (HC31,0) solution. They place 5.00 mL of it in a flask and titrate it with a 0.150 M NaOH solution. At the endpoint of the titration they find that they have used 19.27 mL of the NaOH solution Based on this information answer the following questions. a) How many moles of NaOH are used to reach the endpoint? moles NaOH b) How many moles of acetic...
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.
QUESTION 19 A student is trying to determine the concentration of an acetic acid (HC31,0) solution. They place 5.00 mL of it in a flask and titrate it with a 0.150 M NaOH solution. At the endpoint of the titration they find that they have used 19.27 mL of the NaOH solution Based on this information answer the following questions. a) How many moles of NaOH are used to reach the endpaint? moles NaOH b) How many moles of acetic...
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