What is the equilibrium speciation of free chlorine forms (HOCl, OCl-, and Cl2(aq)) at pH 5.0 in a water containing 35 mg/L of Cl-? Assume that total chlorine is 10-3 M.
What is the equilibrium speciation of free chlorine forms (HOCl, OCl-, and Cl2(aq)) at pH 5.0...
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4. As you know, disinfection of water can be accomplished by bubbling Cl2(g) into the water. the following questions please ignore any influence of water's vapor pressure. In a. (5 points) The Henry's Law Constant for Cl2 is 8.9 x 10 M/Pa (or mol L Pa). If we assume that in this process the pressure of Cl above the water is 101325 Pa, what is the concentration...
Consider a 1.0 L buffer containing 0.109 mol L-1 HOCl and 0.095 mol L-1 OCl-. What is the pH of the solution after adding 7.2 x 10-3 mol of NaOH? Express your answer to 2 decimal places.
24) The hypochlorite ion (OCl-) is a strong oxidizing agent often found in household bleaches and disinfectants. It is also the active ingredient that forms when swimming pool water is treated with chlorine. In addition to its oxidizing abilities, the hypochlorite ion has a relatively high affinity for protons (it is a much stronger base than Cl-, for example) and forms the weakly acidic hypochlorous acid (HOCl, Ka = 3.5 x 10-8). Calculate the pH of a 0.100 M aqueous...
The hypochlorite ion (OCl-) is a strong oxidizing agent often found in household bleaches and disinfectants. It is also the active ingredient that forms when swimming pool water is treated with chlorine. In addition to its oxidizing abilities, the hypochlorite ion has a relatively high affinity for protons (it is a much stronger base than Cl-, for example) and forms the weakly acidic hypochlorous acid (HOCl, Ka = 3.5 x 10-8). Calculate the pH of a 0.100 M aqueous solution...
1) 20. mL sample of 0.20 M HOCl is added to 25.0mL of 0.20M KOH. What is the pH of the solution? -8 HOCl (Ka = 3.5 x 10 ) 2) The ideal pH for the pool is 7.4. What is the ratio of (OCl- ) to (HOCl) needed to maintain the swimming pool at a pH of 7.4? 3) What would be the new pH if you added 0.3 moles of NaOH to 1.0L of the pool water at...
4. If 15 mg/L of HOCl is added to a potable water for disinfection and the final measured pH is 7.0, what percentage of the HOCl is dissociated? Assume the temperature is 25°C and pKa- 7.54. Note that the dissociation of hypochlorous acid proceeds as follows:
4. If 15 mg/L of HOCl is added to a potable water for disinfection and the final measured pH is 7.0, what percentage of the HOCl is dissociated? Assume the temperature is 25°C and...
1. Consider a 1.0 L buffer containing 0.102 mol L-1 HOCl and 0.103 mol L-1 OCl-. What is the pH of the solution after adding 2.8 x 10-3 mol of HCl? Express your answer to 2 decimal places. 2. What is the pH of a solution containing 0.179 mol L-1 HF and 0.329 mol L-1 F- ? Round your answer to 2 decimal places. 3. 15.4 mL solution of 0.100 mol L-1 NaOH is titrated using 0.150 mol L-1 HCl....
Hybrobromous acid, HBrO, is a weak acid. It's acid dissociation constant. Ka is 2.5 x 10-9 a) Calculate the [H+] of a 0.14 molar solution of HBrO b) Write the correctly balanced net ionic equation for the reaction that occurs NaBrO is dissolved in water and calculate the numerical value of the equilibrium constant for this reaction c) Calculate the pH of a solution made by combining 40.0 milliliters of 0.14 molar HBrO and 5.0 milliliters of 0.56 molar NaOH...
A recent study has shown that monochloramne, NH2Cl, “decays” in wastewater is very slow, especially in comparison with free chlorine, HOCl and OCl‐. The exposure of NH2Cl to light was found to increase the rate of decay significantly. When light was completely excluded from the sample, 20 percent decay took place in 8 hours and the data conformed to the first‐order rate law. (a) Assuming (1) a treatment planet is discharging effluent containing 1 mg/L NH2Cl as Cl2; (2) a...
1- In the presence of excess OH-, the Zn2+(aq) ion forms a hydroxide complex ion, Zn(OH)42-. Calculate the concentration of free Zn2+ ion when 1.32×10-2mol ZnSO4(s) is added to 1.00 L of solution in which [OH- ] is held constant (buffered at pH 12.40). For Zn(OH)42-, Kf = 4.6×1017. [Zn2+] = ------ M 2- What is the approximate concentration of free Hg2+ ion at equilibrium when 1.86×10-2 mol mercury(II) nitrate is added to 1.00 L of solution that is 1.310...