Homework Answers
Answer:
a)
Here the deionized water is utilized as the dissolvable.
It is deionized so superfluous particles don't meddle with the response among iodine and hydrogen peroxide(H2O2).
b)
Here buffer is added to keep the pH of the arrangement steady , sodium thiosulfate will be added to stifle the rate of the turn around response.
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3. In the kinetic analysis of this experiment for the reaction of iodide ion with hydrogen...
Key Ouestion #2: Determine the initial concentrations for the following solutions. Solution Preparation Acetic Acid Acetate...
Key Ouestion #2: Determine the initial concentrations for the following solutions. Solution Preparation Acetic Acid Acetate Ion Concentration Concentration Solution #1 50.0 mL of 0.0500 M acetic acid and 0.205 grams of sodium acetate Solution #2 25.0 mL of 0.0500 M acetic acid, 25.0 mL of deionized water, and 0.205 grams of sodium acetate 50.0 mL of 0.0500 M acetic acid and 0.102 grams of sodium acetate Solution #3 Solution # 4 50.0 mL of 0.0500 M acetic acid Solution...
Preparation of Buffer Solutions (2 pts each) Mass of sodium acetate in acetate buffer 1.9821 3.00...
Preparation of Buffer Solutions (2 pts each) Mass of sodium acetate in acetate buffer 1.9821 3.00m 2.0103 Volume of 3.0 M acetic acid in acetate buffer Mass of ammonium chloride Volume of 5.0 M NH4OH pH Mcasurements.Experimental Valucs epts. eachi Deionized Water Ammonia Buffer Acetate Buffer 5 25 4.4 9.12 .33 5.1 23.3 9.04 pH of solution płł of solution after addition of I mL of 0.6 M NaOH pH of solution after addition of 1 mL of 0.6 M...
Please answer all the questions. thank you. Worksheet 4. Which solution in above table has composition...
Please answer all the questions. thank you.
Worksheet 4. Which solution in above table has composition of an ideal buffer? The buffer in this experiment is made of acetic acid HCH.O and sodium acetate NaCHO. (CHO). Ka=1.76 x 10 for HCH:02 Each buffer composition is listed in the table below. 5. If the buffer is mainly used to neutralize added acid (H'), which buffer solution would be most effective? Please explain Test Tube Number Table 1 Solution Reference (Acetic acid)...
Acid buffer described in Problem 21, you discover that your m ion? laboratory is out of sodium ac...
number 23
acid buffer described in Problem 21, you discover that your m ion? laboratory is out of sodium acetate, but you do have sodium hydroxide. How much (in moles and grams) acetic acid and til the pH on of the sodium hydroxide do you need to make the buffer? f th ola . Another alternative. Your friend from another labora- ory was out of acetic acid, so tries to prepare the buffer in Problem 21 by dissolving 41.02 g...
The oxidation of iodide ion by hydrogen peroxide in an acidic solution is described by the...
The oxidation of iodide ion by hydrogen peroxide in an acidic solution is described by the balanced equation H2O2(aq)+3I−(aq)+2H+(aq)⟶I3−(aq)+2H2O(l)H2O2(aq)+3I−(aq)+2H+(aq)⟶I3−(aq)+2H2O(l) The rate of formation of the red triiodide ion, Δ[I3−]/ΔtΔ[I3−]/Δt, can be determined by measuring the rate of appearance of the color. A sequence of photographs showing the progress of the reaction of hydrogen peroxide (H2O2)(H2O2) and iodide ion (I−)(I−). As time passes (left to right), the red color due to the triiodide ion (I3−)(I3−) increases in intensity. Initial rate data...
When solutions of acetic acid and sodium hydroxide react, which of the following are NOT present...
When solutions of acetic acid and sodium hydroxide react, which of the following are NOT present in the complete ionic equation? hydrogen ion hydroxide ion O water sodium ion O acetate ion When solutions of acetic acid and sodium hydroxide react, which of the following are NOT present in the complete ionic equation? hydrogen ion hydroxide ion water O sodium ion acetate non aer 20191121-WA0036.jpg Question 9 If the pH of a salt solution is 5.3, the salt must be...
4. Experimental Procedure, Part A, Table 5.1 a. In Trial 1, what is the function of...
4. Experimental Procedure, Part A, Table 5.1 a. In Trial 1, what is the function of the sodium thiosulfate in studying the kinetics of the hydrogen peroxide-iodide reaction? b. Calculate the moles of S,0,2 that are consumed during the course of the reaction in Trial 1 produced during the course of the reaction. See equation 5.1 that are c. Calculate the moles of I Eveian 3 noitoviioA b d. Calculate the initial molar concentration of I (at time 0), [I...
Chemical Kinetics Kit for AP Chemistry Student Guide d. Is it likely that this reaction occurs...
Chemical Kinetics Kit for AP Chemistry Student Guide d. Is it likely that this reaction occurs in one step? Explain. 2. A student would like to determine the orders of the reaction for an iodine clock reaction that occurs in three steps 3r(aq)+ H,O:(aq) + 2H'(aq )-,(aq) +2H 2O0) slow I(aq) + 25,0,(aq) 3r(aq) + S40(aq) 21, (aq) + starch-starch-I" complex + r(aq) fast fast Write the rate law for this reaction, using variables in place of the exponents a...
Write balanced reaction for: a) Iron(III) ion with excess of ammonia in aqueous solution b) Copper(II)...
Write balanced reaction for: a) Iron(III) ion with excess of ammonia in aqueous solution b) Copper(II) ion with excess of ammonia in aqueous solution c) The reaction between copper(II) nitrate and potassium iodide d) The oxidation of chromium(III) to chromate(VI) with hydrogen peroxide in sodium hydroxide solution
Calculations The following calculations are necessary to complete your Report Sheet. Consult the table on page...
Calculations The following calculations are necessary to complete your Report Sheet. Consult the table on page 119 for appropriate K and K, values. Complete these calculations on your Report Sheet for complete credit. I. pH of Strong and Weak Acids 1. Calculate the pH of a 0.10 M hydrochloric acid solution, HCl(aq). 2. Calculate the pH of a solution prepared by diluting 5.00 mL of 0.10 M hydrochloric acid, HCl (aq), in enough water to make a 50.0 mL solution....
Key Ouestion #2: Determine the initial concentrations for the following solutions. Solution Preparation Acetic Acid Acetate Ion Concentration Concentration Solution #1 50.0 mL of 0.0500 M acetic acid and 0.205 grams of sodium acetate Solution #2 25.0 mL of 0.0500 M acetic acid, 25.0 mL of deionized water, and 0.205 grams of sodium acetate 50.0 mL of 0.0500 M acetic acid and 0.102 grams of sodium acetate Solution #3 Solution # 4 50.0 mL of 0.0500 M acetic acid Solution...
Preparation of Buffer Solutions (2 pts each) Mass of sodium acetate in acetate buffer 1.9821 3.00m 2.0103 Volume of 3.0 M acetic acid in acetate buffer Mass of ammonium chloride Volume of 5.0 M NH4OH pH Mcasurements.Experimental Valucs epts. eachi Deionized Water Ammonia Buffer Acetate Buffer 5 25 4.4 9.12 .33 5.1 23.3 9.04 pH of solution płł of solution after addition of I mL of 0.6 M NaOH pH of solution after addition of 1 mL of 0.6 M...
Please answer all the questions. thank you.
Worksheet 4. Which solution in above table has composition of an ideal buffer? The buffer in this experiment is made of acetic acid HCH.O and sodium acetate NaCHO. (CHO). Ka=1.76 x 10 for HCH:02 Each buffer composition is listed in the table below. 5. If the buffer is mainly used to neutralize added acid (H'), which buffer solution would be most effective? Please explain Test Tube Number Table 1 Solution Reference (Acetic acid)...
number 23
acid buffer described in Problem 21, you discover that your m ion? laboratory is out of sodium acetate, but you do have sodium hydroxide. How much (in moles and grams) acetic acid and til the pH on of the sodium hydroxide do you need to make the buffer? f th ola . Another alternative. Your friend from another labora- ory was out of acetic acid, so tries to prepare the buffer in Problem 21 by dissolving 41.02 g...
When solutions of acetic acid and sodium hydroxide react, which of the following are NOT present in the complete ionic equation? hydrogen ion hydroxide ion O water sodium ion O acetate ion When solutions of acetic acid and sodium hydroxide react, which of the following are NOT present in the complete ionic equation? hydrogen ion hydroxide ion water O sodium ion acetate non aer 20191121-WA0036.jpg Question 9 If the pH of a salt solution is 5.3, the salt must be...
4. Experimental Procedure, Part A, Table 5.1 a. In Trial 1, what is the function of the sodium thiosulfate in studying the kinetics of the hydrogen peroxide-iodide reaction? b. Calculate the moles of S,0,2 that are consumed during the course of the reaction in Trial 1 produced during the course of the reaction. See equation 5.1 that are c. Calculate the moles of I Eveian 3 noitoviioA b d. Calculate the initial molar concentration of I (at time 0), [I...
Chemical Kinetics Kit for AP Chemistry Student Guide d. Is it likely that this reaction occurs in one step? Explain. 2. A student would like to determine the orders of the reaction for an iodine clock reaction that occurs in three steps 3r(aq)+ H,O:(aq) + 2H'(aq )-,(aq) +2H 2O0) slow I(aq) + 25,0,(aq) 3r(aq) + S40(aq) 21, (aq) + starch-starch-I" complex + r(aq) fast fast Write the rate law for this reaction, using variables in place of the exponents a...
Calculations The following calculations are necessary to complete your Report Sheet. Consult the table on page 119 for appropriate K and K, values. Complete these calculations on your Report Sheet for complete credit. I. pH of Strong and Weak Acids 1. Calculate the pH of a 0.10 M hydrochloric acid solution, HCl(aq). 2. Calculate the pH of a solution prepared by diluting 5.00 mL of 0.10 M hydrochloric acid, HCl (aq), in enough water to make a 50.0 mL solution....
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