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What mass of sodium hypochlorite, NaOCI (molar mass 74.5...
A solution of household bleach contains 5.25% sodium hypochlorite, NaOCI, by mass
A solution of household bleach contains 5.25% sodium hypochlorite, NaOCI, by mass. Assuming that the density of bleach is the same as water, calculate the volume of household bleach that should be diluted with water to make 500 0 mL of a pH = 10.26 solution. Use the Ka of hypochlorous acid found in the chempendix.
Part 1: Buffers Considering the acetic acid sodium acetate buffer, complete the table below NaOH added/mL....
Part 1: Buffers Considering the acetic acid sodium acetate buffer, complete the table below NaOH added/mL. measured pH 0.0 20 Did the pH change a little or a lot when NaOH was added to the butter? Was the change you observed consistent with the action of a butter? For the ammonium chloride-ammonia buffer give the measured pH for the 50.0 mL of 0.10 Mammonia. Is this solution acidic, neutral, or basic? Did the pH of the ammonia increase or decrease...
A buffer solution of hypochlorous acid HOCI and sodium hypochlorite NaOCI was created by combining 0.76...
A buffer solution of hypochlorous acid HOCI and sodium hypochlorite NaOCI was created by combining 0.76 mol HOCI with 0.87 mol NaOCl in a total volume of 3.5 L. The Ka of hypochlorous acid is 3.0 x 10-8 at 25°C. Determine the pH of this buffer solution at 25°C. 11
The pK, of hypochlorous acid is 7.530. A 56.0 mL solution of 0.142 M sodium hypochlorite (NaOCI) is titrated w...
The pK, of hypochlorous acid is 7.530. A 56.0 mL solution of 0.142 M sodium hypochlorite (NaOCI) is titrated with 0.292 MHCI. Calculate the pH of the solution after the addition of 8.44 mL of 0.292 M HCI. pH = Calculate the pH of the solution after the addition of 28.6 ml of 0.292 M HCI. pH = Calculate the pH of the solution at the equivalence point with 0.292 M HCI. pH =
The pK, of hypochlorous acid is 7.530. A 55.0 mL solution of 0.116 M sodium hypochlorite...
The pK, of hypochlorous acid is 7.530. A 55.0 mL solution of 0.116 M sodium hypochlorite (NaOCI) is titrated with 0.252 M HCI. Calculate the pH of the solution after the addition of 9.37 mL of 0.252 M HCL. pH = Calculate the pH of the solution after the addition of 26.6 ml of 0.252 M HCI. pH = Calculate the pH of the solution at the equivalence point with 0.262 M HCI. pH =
The pK, of hypochlorous acid is 7.530. A 57.0 mL solution of 0.129 M sodium hypochlorite...
The pK, of hypochlorous acid is 7.530. A 57.0 mL solution of 0.129 M sodium hypochlorite (NaOCI) is titrated with 0.312 MHCI. Calculate the pH of the solution after the addition of 7.38 mL of 0.312 M HCI. pH = Calculate the pH of the solution after the addition of 25.0 mL of 0.312 M HCI. pH = Calculate the pH of the solution at the equivalence point with 0.312 M HCl. pH =
7&8 please? Thanks! 1. What is the pH of a 0.120 M solution of NH3(aq)? For...
7&8 please? Thanks!
1. What is the pH of a 0.120 M solution of NH3(aq)? For ammonia, Kb=1./TIU. 8. Sodium hypochlorite, NaOCI, is the active ingredient in chlorine bleach (e.g., Chlorox). For hypochlorous acid, HOCI with Ka=3.0x10-8. a. Write the equation for the base hydrolysis equilibrium of the hypochlorite ion. b. What is the value of Kb for the hypochlorite ion? CHEM 1474 General Chemistry II c. What is the pH of a 0.10 M solution of sodium hypochlorite?
A 1.00 liter solution contains 0.53 moles hypochlorous acid and 0.41 moles potassium hypochlorite. If 0.20...
A 1.00 liter solution contains 0.53 moles hypochlorous acid and 0.41 moles potassium hypochlorite. If 0.20 moles of hydrobromic acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydrobromic acid.) A. The number of moles of HCIO will remain the same. B. The number of moles of CIO will remain the same. C. The equilibrium concentration of H,0* will decrease. D. The pH...
A solution was prepared by dissolving 0.200 moles of sodium hypoch lorite (NaClO) in water to...
A solution was prepared by dissolving 0.200 moles of sodium hypoch lorite (NaClO) in water to a final volume of 1.00 Liter. Ka 2.96x10 for hypochlorous acid (HCIO). Show equations and work steps for these calculations. 1) Calculate Kb of sodium hypochlorite. 2) Calculate the pH of the NaClO solution. 3) Calculate the pH if 10.0 mL of 1.00 M HCl is added to 100.0 mL of the original NACIO solution. 4) Calculate the pH if 20.0 mL of 1.00...
Determination of Ka and Identification of an Unknown Weak Acid Post-lab Question 1. Suppose that a student performi...
Determination of Ka and Identification of an Unknown Weak Acid Post-lab Question 1. Suppose that a student performing this experiment mistakenly calibrated the pH meter using pH 8 buffer instead of pH 7 buffer. As a result of this error, all of the student's pH readings were too low. a) Would this error have affected the calculated molar mass of the unknown acid? Briefly explain. b) Would this error have affected the experimentally determined pKa of the unknown acid? Briefly...
Part 1: Buffers Considering the acetic acid sodium acetate buffer, complete the table below NaOH added/mL. measured pH 0.0 20 Did the pH change a little or a lot when NaOH was added to the butter? Was the change you observed consistent with the action of a butter? For the ammonium chloride-ammonia buffer give the measured pH for the 50.0 mL of 0.10 Mammonia. Is this solution acidic, neutral, or basic? Did the pH of the ammonia increase or decrease...
A buffer solution of hypochlorous acid HOCI and sodium hypochlorite NaOCI was created by combining 0.76 mol HOCI with 0.87 mol NaOCl in a total volume of 3.5 L. The Ka of hypochlorous acid is 3.0 x 10-8 at 25°C. Determine the pH of this buffer solution at 25°C. 11
The pK, of hypochlorous acid is 7.530. A 56.0 mL solution of 0.142 M sodium hypochlorite (NaOCI) is titrated with 0.292 MHCI. Calculate the pH of the solution after the addition of 8.44 mL of 0.292 M HCI. pH = Calculate the pH of the solution after the addition of 28.6 ml of 0.292 M HCI. pH = Calculate the pH of the solution at the equivalence point with 0.292 M HCI. pH =
The pK, of hypochlorous acid is 7.530. A 55.0 mL solution of 0.116 M sodium hypochlorite (NaOCI) is titrated with 0.252 M HCI. Calculate the pH of the solution after the addition of 9.37 mL of 0.252 M HCL. pH = Calculate the pH of the solution after the addition of 26.6 ml of 0.252 M HCI. pH = Calculate the pH of the solution at the equivalence point with 0.262 M HCI. pH =
The pK, of hypochlorous acid is 7.530. A 57.0 mL solution of 0.129 M sodium hypochlorite (NaOCI) is titrated with 0.312 MHCI. Calculate the pH of the solution after the addition of 7.38 mL of 0.312 M HCI. pH = Calculate the pH of the solution after the addition of 25.0 mL of 0.312 M HCI. pH = Calculate the pH of the solution at the equivalence point with 0.312 M HCl. pH =
7&8 please? Thanks!
1. What is the pH of a 0.120 M solution of NH3(aq)? For ammonia, Kb=1./TIU. 8. Sodium hypochlorite, NaOCI, is the active ingredient in chlorine bleach (e.g., Chlorox). For hypochlorous acid, HOCI with Ka=3.0x10-8. a. Write the equation for the base hydrolysis equilibrium of the hypochlorite ion. b. What is the value of Kb for the hypochlorite ion? CHEM 1474 General Chemistry II c. What is the pH of a 0.10 M solution of sodium hypochlorite?
A 1.00 liter solution contains 0.53 moles hypochlorous acid and 0.41 moles potassium hypochlorite. If 0.20 moles of hydrobromic acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydrobromic acid.) A. The number of moles of HCIO will remain the same. B. The number of moles of CIO will remain the same. C. The equilibrium concentration of H,0* will decrease. D. The pH...
A solution was prepared by dissolving 0.200 moles of sodium hypoch lorite (NaClO) in water to a final volume of 1.00 Liter. Ka 2.96x10 for hypochlorous acid (HCIO). Show equations and work steps for these calculations. 1) Calculate Kb of sodium hypochlorite. 2) Calculate the pH of the NaClO solution. 3) Calculate the pH if 10.0 mL of 1.00 M HCl is added to 100.0 mL of the original NACIO solution. 4) Calculate the pH if 20.0 mL of 1.00...
Determination of Ka and Identification of an Unknown Weak Acid Post-lab Question 1. Suppose that a student performing this experiment mistakenly calibrated the pH meter using pH 8 buffer instead of pH 7 buffer. As a result of this error, all of the student's pH readings were too low. a) Would this error have affected the calculated molar mass of the unknown acid? Briefly explain. b) Would this error have affected the experimentally determined pKa of the unknown acid? Briefly...
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