Homework Answers
a) Phenolphthalein is used as an indicator in acid base titration . By changing the colour phenolphthalein shows us the medium of solution
Neutral medium :- Colourless
Acidic medium :- colourless
Basic medium :- Pink
b ) we look for colourless ( acidic ) to pink colour
( basic ) change for the end point
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7. You are given a solution of unknown concentration of HCI. (8 Points) You are asked...
Question 1 include A, B & C I want to produce nitric acid, HNO3 using the...
Question 1 include A, B & C
I want to produce nitric acid, HNO3 using the unbalanced reaction below. In the lab I have 250ml of a 0.50M solution of barium nitrate. Ba(NO3)2 + H2S →BaS + HNO3. A. Balance the reaction? B. How many moles of Barium nitrated do I have? C. How many moles of nitric acid is it possible to produce? D. Assuming the final volume is the same as the volume of barium nitrate used, what...
3. A student pipetted 25.00 mL of a 0.2531 M solution of HCl into an Erlenmeyer...
3. A student pipetted 25.00 mL of a 0.2531 M solution of HCl into an Erlenmeyer flask. After adding 3 drops of phenolphthalein indicator to the flask, the student started adding NaOH from the burette, until the color in the Erlenmeyer flask turned light pink, The student calculated that 21.40 mL NaOH was transferred in the flask to neutralize the acid. a) Calculate the number of moles of HCl initially present (Reaction: NaOH(aq) + HCl(aq) -NaCl(aq) + H2O() b) Calculate...
Question 40 of 65 > The flask contains 10.0 mL of HCl and a few drops...
Question 40 of 65 > The flask contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.140 M NaOH. It requires 12.8 mL of the NaOH solution to reach the end point of the titration. What is the initial concentration of HCI? concentration: MHCI
Determine how many liters (l) of stock HCl were used in titration #1. Please fill all...
Determine how many liters (l) of stock HCl were used
in titration #1.
Please fill all questions under "Data Analysis"
Page 1 is just instruction for Page 2
EXPT 10: TITRATION OF STRONG ACID WITH STRONG BASE Note to Students: when you see the symbol (), this means there is something you must add into the mock data yourself. You may handwrite or type your answers directly on these pages for submission to a Blackboard link. Remember to show all...
Concentration of Standardized HCI Solution = 0.39 Flask Mass Mg (g) 0.0845 0.0815 Volume HCI (mL)...
Concentration of Standardized HCI Solution = 0.39 Flask Mass Mg (g) 0.0845 0.0815 Volume HCI (mL) T 10mL 10mL 12.15 m2 Initial volume NaOH (mL) 21.15ML Final volume NaOH (ml) 21. 15m2 31.5mL Volume used NaOH (mL) 19 mL 10.35 ml CALCULATIONS **Show work for each trial.** . Moles of Mg used • Initial moles of HCl (total moles of HCl placed into each Erlenmeyer flask) • Moles of NaOH Moles of HCl titrated NaOH + HCI -----> NaCl +...
The flask contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret...
The flask contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.210 M NaOH. It requires 16.4 mL of the NaOH solution to reach the end point of the titration. What is the initial concentration of HCI? concentration: MHCI URILE
Data the experiment Record For the lab report, attach this data sheet (signed by your TA) to your...
please write out calculations for each box missing an answer
data the experiment Record For the lab report, attach this data sheet (signed by your TA) to your calculations page. REPORT ALL VALUES TO AT LEAST THREE SIGNIFICANT FIGURES. READ YOUR BURETTE TO THE NEAREST 0.05 mL increment. for on this sheet. Do your calculations on a separate piece of paper. Part One-Standardization of a NaOH solution of approximately 0.1 M. Trial 1 | Trial 2 | Trial 3 Mass...
Concentration of Standardized HCI Solution = 0.934 M Flask 2 Mass Mg (8) 10.0849 0.0815 Volume...
Concentration of Standardized HCI Solution = 0.934 M Flask 2 Mass Mg (8) 10.0849 0.0815 Volume HCI (mL) I 10mL 10mL Initial volume NaOH (mL) 12.15ml Final volume NaOH (mL) 21.154L 9 m 21. 15ML 31.5mL 10.35 mL Volume used NaOH (mL) CALCULATIONS **Show work for each trial.** • Moles of Mg used Trial 0.084 Hy loola 10.001g Mg = 0.00 0.003375 mol My 0.0035 molto • Initial moles of HCl (total moles of HCl placed into each Erlenmeyer flask)...
QUESTION 1 6 points Save Answer The purpose of an indicator in an acid-base titration is...
QUESTION 1 6 points Save Answer The purpose of an indicator in an acid-base titration is to indicate the of the titration. Use Table 10.2 for the following question. If an acidic solution is titrated with a basic solution and methyl violet is used as an indicator, the solution color will change from to QUESTION 2 3 points Save Answer The molarity of a solution prepared by dissolving 17.0 g of hydrochloric acid (HCI (aq) in 133 mL of water...
There will be a short quiz held at the beginning of the lab session. The quiz...
There will be a short quiz held at the beginning of the lab session. The quiz will be based on some of the material shown below. 1. A student performed a titration on a 5.00 mL sample of an unknown HCl solution, using 10.90 mL of 0.09345 M NaOH from a buret and phenolphthalein indicator. What was the concentration of the unknown HCI? Use the correct number of sign ificant figures. 2. Another student designed a procedure to determine the...
Question 1 include A, B & C
I want to produce nitric acid, HNO3 using the unbalanced reaction below. In the lab I have 250ml of a 0.50M solution of barium nitrate. Ba(NO3)2 + H2S →BaS + HNO3. A. Balance the reaction? B. How many moles of Barium nitrated do I have? C. How many moles of nitric acid is it possible to produce? D. Assuming the final volume is the same as the volume of barium nitrate used, what...
3. A student pipetted 25.00 mL of a 0.2531 M solution of HCl into an Erlenmeyer flask. After adding 3 drops of phenolphthalein indicator to the flask, the student started adding NaOH from the burette, until the color in the Erlenmeyer flask turned light pink, The student calculated that 21.40 mL NaOH was transferred in the flask to neutralize the acid. a) Calculate the number of moles of HCl initially present (Reaction: NaOH(aq) + HCl(aq) -NaCl(aq) + H2O() b) Calculate...
Question 40 of 65 > The flask contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.140 M NaOH. It requires 12.8 mL of the NaOH solution to reach the end point of the titration. What is the initial concentration of HCI? concentration: MHCI
Determine how many liters (l) of stock HCl were used
in titration #1.
Please fill all questions under "Data Analysis"
Page 1 is just instruction for Page 2
EXPT 10: TITRATION OF STRONG ACID WITH STRONG BASE Note to Students: when you see the symbol (), this means there is something you must add into the mock data yourself. You may handwrite or type your answers directly on these pages for submission to a Blackboard link. Remember to show all...
Concentration of Standardized HCI Solution = 0.39 Flask Mass Mg (g) 0.0845 0.0815 Volume HCI (mL) T 10mL 10mL 12.15 m2 Initial volume NaOH (mL) 21.15ML Final volume NaOH (ml) 21. 15m2 31.5mL Volume used NaOH (mL) 19 mL 10.35 ml CALCULATIONS **Show work for each trial.** . Moles of Mg used • Initial moles of HCl (total moles of HCl placed into each Erlenmeyer flask) • Moles of NaOH Moles of HCl titrated NaOH + HCI -----> NaCl +...
The flask contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.210 M NaOH. It requires 16.4 mL of the NaOH solution to reach the end point of the titration. What is the initial concentration of HCI? concentration: MHCI URILE
please write out calculations for each box missing an answer
data the experiment Record For the lab report, attach this data sheet (signed by your TA) to your calculations page. REPORT ALL VALUES TO AT LEAST THREE SIGNIFICANT FIGURES. READ YOUR BURETTE TO THE NEAREST 0.05 mL increment. for on this sheet. Do your calculations on a separate piece of paper. Part One-Standardization of a NaOH solution of approximately 0.1 M. Trial 1 | Trial 2 | Trial 3 Mass...
Concentration of Standardized HCI Solution = 0.934 M Flask 2 Mass Mg (8) 10.0849 0.0815 Volume HCI (mL) I 10mL 10mL Initial volume NaOH (mL) 12.15ml Final volume NaOH (mL) 21.154L 9 m 21. 15ML 31.5mL 10.35 mL Volume used NaOH (mL) CALCULATIONS **Show work for each trial.** • Moles of Mg used Trial 0.084 Hy loola 10.001g Mg = 0.00 0.003375 mol My 0.0035 molto • Initial moles of HCl (total moles of HCl placed into each Erlenmeyer flask)...
QUESTION 1 6 points Save Answer The purpose of an indicator in an acid-base titration is to indicate the of the titration. Use Table 10.2 for the following question. If an acidic solution is titrated with a basic solution and methyl violet is used as an indicator, the solution color will change from to QUESTION 2 3 points Save Answer The molarity of a solution prepared by dissolving 17.0 g of hydrochloric acid (HCI (aq) in 133 mL of water...
There will be a short quiz held at the beginning of the lab session. The quiz will be based on some of the material shown below. 1. A student performed a titration on a 5.00 mL sample of an unknown HCl solution, using 10.90 mL of 0.09345 M NaOH from a buret and phenolphthalein indicator. What was the concentration of the unknown HCI? Use the correct number of sign ificant figures. 2. Another student designed a procedure to determine the...
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