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Question 10 (1 point) Common "pool acid", that can be purchased at any hardware store, is...
need help with all stine Hydrochloric Acid Solution with a Standard Sodium Hydroxide Solution ANAL. 425:...
need help with all
stine Hydrochloric Acid Solution with a Standard Sodium Hydroxide Solution ANAL. 425: Titrating Hydrochloric Acid Sol Post-Laboratory Questions se the spaces provided for the answers and additional paper if necessary) UUUUUUUUUUUUU (4) Briefly comment on the procedural problem associated with the titration described in (3). 1. A chemistry student purchased commercially pre- pared muriatic acid for use in cleaning a home swim- ming pool. Realizing that muriatic acid is another name for HCl solution, the student...
ANAL 425: Titrating Hydrochloric Acid Solution with a Standard Sodium Hydroxide Solution ANAL 42: The Hydrochlork...
ANAL 425: Titrating Hydrochloric Acid Solution with a
Standard Sodium Hydroxide Solution
ANAL 42: The Hydrochlork Acil Solution with Standard Sodium Hydroxide Solution (3) Calculate the number of equivalents of acid in 1.00 lb of dry acid powder. The molar mass of NaHSO, is 120.07 g mol (4) Calculate the mass, in pounds, of dry acid powder required to supply the equivalent amount of acid present in 1 qt (0.9463 L) of the commercial muri- atic acid solution discussed in...
can i get help with this question please 3. Consider the weak base-strong acid titration of...
can i get help with this question please
3. Consider the weak base-strong acid titration of 25.00 mL of 0.100 M NH, with 0.100 M HCl (weak base, strong acid). The Ks for this weak base is 1.8 x 10 a. Calculate the pH of the solution after the addition of 10.0 mL HCL. b. What is the pH half-way to the equivalence point? c. Calculate the pH at the equivalence point. d. Calculate the pH after the addition of...
Can anyone please help with how to calculate degree of ionization for the first 3 solutions...
Can anyone please help with how to calculate degree of
ionization for the first 3 solutions as well as how to calculate
the expected pH for solution 4? thank you!
Experiment 8: Equilibria of Weak Acids and Bases Lab Report Sheet 1 Composition 20.0 mL of 0.1 M HC2H302 - (A weak acid) pH 12.76 2.42 2.59 10.0 mL of 0.10 M HC2H3O2 + 10.0 mL H20 - (effect of dilution on the degree of ionization of weak acid) 10.0...
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...
Match the question with the best answer: A. 2x 10-14 В. -log Ka C. pH 7...
Match the question with the best answer:
A. 2x 10-14 В. -log Ka C. pH 7 D. hydrogen ion donor рн E. water F. hydrogen ion acceptor рКа G. H30 OH т рКw H. -log [OH Concentration of [OH] in pure water 1. Ка т Кw Bronsted acid J.1 x 107 M Bronsted base К. 14 L. pH 7 Can act as both an acid and a base М. Кь N. 1 x 1014 O. -log [H30*] Р. рн <7
How could you make 2.5 L of 0.10 M hydrochloric acid? Question 10 (1 point) How...
How could you make 2.5 L of 0.10 M hydrochloric acid?
Question 10 (1 point) How could you make 2.5 L of 0.10 M hydrochloric acid? Hint: This is a dilution. How many moles of HCI in 2.5L of 0.1M? Use the fact that M = ? that M - n moles so # of moles n = M, V =.. O dilute 59.4 mL of 3.0 M HCl to 2.5 L with water O dilute 0.25 L of pure...
1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2....
1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCl stock solution. In your response to this question, be very specific about the quantities of stock solution and deionized water to be used in the dilution and the...
Titration: Acids and Bases 2. How can you determine which acid is diprotic? 3. using the...
Titration: Acids and Bases
2. How can you determine which acid is diprotic?
3. using the answers to questions one and two, which acid is
diprotic?
4. Which base has more hydroxide ions per molecule?
Acid Volume Base Base Initial Volume (mL) Base Final Volume (mL) Volume of Base Used (mL) Acid: Base Ratio Acid 1 20 mL Base 1 50 mL 34.5 15.5 4:3 Acid 2 20 mL Base 1 Acid 1 20 mL Base 2 Acid 2 20...
Question 7 (1 point) Vitamin C is a more common name for ascorbic acid (Ka -...
Question 7 (1 point) Vitamin C is a more common name for ascorbic acid (Ka - 8.0 x 10-5). Calculate the pH of a 0.034 M solution of vitamin C. 04.10 8.43 O 5.57 O 11.22 2.78
need help with all
stine Hydrochloric Acid Solution with a Standard Sodium Hydroxide Solution ANAL. 425: Titrating Hydrochloric Acid Sol Post-Laboratory Questions se the spaces provided for the answers and additional paper if necessary) UUUUUUUUUUUUU (4) Briefly comment on the procedural problem associated with the titration described in (3). 1. A chemistry student purchased commercially pre- pared muriatic acid for use in cleaning a home swim- ming pool. Realizing that muriatic acid is another name for HCl solution, the student...
ANAL 425: Titrating Hydrochloric Acid Solution with a
Standard Sodium Hydroxide Solution
ANAL 42: The Hydrochlork Acil Solution with Standard Sodium Hydroxide Solution (3) Calculate the number of equivalents of acid in 1.00 lb of dry acid powder. The molar mass of NaHSO, is 120.07 g mol (4) Calculate the mass, in pounds, of dry acid powder required to supply the equivalent amount of acid present in 1 qt (0.9463 L) of the commercial muri- atic acid solution discussed in...
can i get help with this question please
3. Consider the weak base-strong acid titration of 25.00 mL of 0.100 M NH, with 0.100 M HCl (weak base, strong acid). The Ks for this weak base is 1.8 x 10 a. Calculate the pH of the solution after the addition of 10.0 mL HCL. b. What is the pH half-way to the equivalence point? c. Calculate the pH at the equivalence point. d. Calculate the pH after the addition of...
Can anyone please help with how to calculate degree of
ionization for the first 3 solutions as well as how to calculate
the expected pH for solution 4? thank you!
Experiment 8: Equilibria of Weak Acids and Bases Lab Report Sheet 1 Composition 20.0 mL of 0.1 M HC2H302 - (A weak acid) pH 12.76 2.42 2.59 10.0 mL of 0.10 M HC2H3O2 + 10.0 mL H20 - (effect of dilution on the degree of ionization of weak acid) 10.0...
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...
Match the question with the best answer:
A. 2x 10-14 В. -log Ka C. pH 7 D. hydrogen ion donor рн E. water F. hydrogen ion acceptor рКа G. H30 OH т рКw H. -log [OH Concentration of [OH] in pure water 1. Ка т Кw Bronsted acid J.1 x 107 M Bronsted base К. 14 L. pH 7 Can act as both an acid and a base М. Кь N. 1 x 1014 O. -log [H30*] Р. рн <7
How could you make 2.5 L of 0.10 M hydrochloric acid?
Question 10 (1 point) How could you make 2.5 L of 0.10 M hydrochloric acid? Hint: This is a dilution. How many moles of HCI in 2.5L of 0.1M? Use the fact that M = ? that M - n moles so # of moles n = M, V =.. O dilute 59.4 mL of 3.0 M HCl to 2.5 L with water O dilute 0.25 L of pure...
1. What is the definition of an 'equivalence point' in an acid/base titration? (1 point) 2. In part one of the experiment, you will prepare the acid solutions being titrated from a stock solution. Describe how you will accurately prepare 10.00 mL of 0.100 M HCl solution using a 1.00 M HCl stock solution. In your response to this question, be very specific about the quantities of stock solution and deionized water to be used in the dilution and the...
Titration: Acids and Bases
2. How can you determine which acid is diprotic?
3. using the answers to questions one and two, which acid is
diprotic?
4. Which base has more hydroxide ions per molecule?
Acid Volume Base Base Initial Volume (mL) Base Final Volume (mL) Volume of Base Used (mL) Acid: Base Ratio Acid 1 20 mL Base 1 50 mL 34.5 15.5 4:3 Acid 2 20 mL Base 1 Acid 1 20 mL Base 2 Acid 2 20...
Question 7 (1 point) Vitamin C is a more common name for ascorbic acid (Ka - 8.0 x 10-5). Calculate the pH of a 0.034 M solution of vitamin C. 04.10 8.43 O 5.57 O 11.22 2.78
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