## Info

13.6 The concentration spFeII is determined to be 6.981(10 ) mg/L. The dissolved solids are 140 mg/L and the temperature is 25°C. Although the activity coefficient of FeOH+ ion can be obtained from the knowledge of the dissolved solids content, calculate it using values of the other parameters. The optimum pH is 11.95.

13.7 The optimum pH for precipitating Mn(OH)2 is 11.97 and the dissolved solids content of the water is 140 mg/L. The temperature is 25°C. Calculate the activity coefficient of the hydrogen ion. The data on dissolved solids may be used to calculate other parameters but not for the activity coefficient of the hydrogen ion.

13.8 The optimum pH for precipitating Mn(OH)2 is 11.97 and the dissolved solids content of the water is 140 mg/L. The temperature is 25°C. Calculate the ion product of water. The given temperature may be used to calculate other parameters but not for the ion product.

13.9 The optimum pH for precipitating Mn(OH)2 is 11.97 and the dissolved solids content of the water is 140 mg/L. The temperature is 25°C. Calculate the activity coefficient of the Mn(II) ion. The data on dissolved solids may be used to calculate other parameters but not for the activity coefficient of the manganese ion.

13.10 The optimum pH for precipitating Mn(OH)2 is 11.97 and the dissolved solids content of the water is 140 mg/L. The temperature is 25°C. Calculate the equilibrium constant of Mn (OH) -. The given temperature may used to calculate other parameters but not for the equilibrium constant of Mn( OH)-.

13.11 The optimum pH for precipitating Mn(OH)2 is 11.97 and the dissolved solids content of the water is 140 mg/L. The temperature is 25°C. Calculate the activity coefficient of the Mn( OH) - complex ion. The data on dissolved solids may be used to calculate other parameters but not for the activity coefficient of Mn(OH)3.

13.12 The optimum pH for precipitating Mn(OH)2 is 11.97 and the dissolved solids content of the water is 140 mg/L. The temperature is 25°C. Calculate the equilibrium constant of Mn(OH)+. The given temperature may used to calculate other parameters but not for the equilibrium constant of Mn(OH)+.

13.13 The optimum pH for precipitating Mn(OH)2 is 11.97 and the dissolved solids content of the water is 140 mg/L. The temperature is 25°C. Calculate the activity coefficient of the Mn(OH)+ complex ion. The data on dissolved solids may be used to calculate other parameters but not for the activity coefficient of Mn(OH)+.

13.14 At a pH of 11.97 and a dissolved solids of 140 mg/L, the concentration of spM is 0.0179 mg/L. Calculate the solubility product constant of Mn(OH)2(s). The temperature is 25°C. This given temperature may be used to calculate other parameters but not for the solubility product constant.

13.15 At a pH of 11.97 and dissolved solids of 140 mg/L, the concentration of spMn is 0.0179 mg/L. Calculate the activity coefficient of the hydrogen ion. The temperature is 25°C. The data on dissolved solids may be used to calculate other parameters but not to calculate the activity coefficient of the hydrogen ion.

13.16 At a pH of 11.97 and dissolved solids of 140 mg/L, the concentration of spMn is 0.0179 mg/L. Calculate the equilibrium constant of Mn(OH)+. The temperature is 25°C. This given temperature may be used to calculate other parameters but not the equilibrium constant of Mn(OH)+.

13.17 At a pH of 11.97 and dissolved solids of 140 mg/L, the concentration of spMn is 0.0179 mg/L. Calculate the activity coefficient of Mn(OH)+. The temperature is 25°C. The data on dissolved solids may be used to calculate other parameters but not to calculate the activity coefficient of Mn(OH)+.

13.18 At a pH of 11.97 and dissolved solids of 140 mg/L, the concentration of spMn is 0.0179 mg/L. Calculate the equilibrium constant of Mn (OH)-.

The temperature is 25°C. This given temperature may be used to calculate other parameters but not the equilibrium constant of Mn( OH) -.

13.19 At a pH of 11.97 and dissolved solids of 140 mg/L, the concentration of spMn is 0.0179 mg/L. Calculate the activity coefficient of Mn(OH)-. The temperature is 25°C. The data on dissolved solids may be used to calculate other parameters but not to calculate the activity coefficient of Mn( OH)-.

13.20 At a pH of 11.97 and dissolved solids of 140 mg/L, the concentration of spMn is 0.0179 mg/L. Calculate the ion product of water. The temperature is 25°C. This given temperature may be used to calculate other parameters but not the ion product of water.

13.21 The kilograms of lime per cubic meter needed to meet the limit concentration of 0.05 mg/L is 0.00071. This removal is done at the high pH range. Calculate the concentration of manganese in the raw water.

13.22 The kilograms of lime per cubic meter needed to meet the limit concentration of 0.05 mg/L is 0.0014. This removal is done at the high pH range and the concentration of manganese in the raw water is 2.5 mg/L. Calculate the volume of water treated.

13.23 A raw water contains 2.5 mg/L Mn. Calculate the kilograms of caustic used per cubic meter needed to meet the limit concentration of 0.05 mg/L.

13.24 A raw water contains 2.5 mg/L Mn. Calculate the kilograms of chlorine per cubic meter needed to meet the limit concentration of 0.05 mg/L.

13.25 A raw water contains 2.5 mg/L Mn. Calculate the kilograms of sodium hypochlorite per cubic meter needed to meet the limit concentration of 0.05 mg/L.

13.26 A raw water contains 2.5 mg/L Mn. Calculate the kilograms of calcium hypochlorite per cubic meter needed to meet the limit concentration of 0.05 mg/L.

13.27 A raw water contains 2.5 mg/L Mn. Calculate the kilograms of ozone per cubic meter needed to meet the limit concentration of 0.05 mg/L.

13.28 A raw water contains 2.5 mg/L Mn. Calculate the kilograms of dissolved oxygen per cubic meter needed to meet the limit concentration of 0.05 mg/L.

13.29 A raw water contains 40 mg/L ferrous. Calculate the kilograms of caustic used per cubic meter needed to meet the limit concentration of 0.3 mg/L.

13.30 A raw water contains 40 mg/L ferrous. Calculate the kilograms of chlorine per cubic meter needed to meet the limit concentration of 0.3 mg/L.

13.31 A raw water contains 40 mg/L ferrous. Calculate the kilograms of sodium hypochlorite per cubic meter needed to meet the limit concentration of 0.3 mg/L.

13.32 A raw water contains 40 mg/L ferrous. Calculate the kilograms of calcium hypochlorite per cubic meter needed to meet the limit concentration of 0.3 mg/L.

13.33 A raw water contains 40 mg/L ferrous. Calculate the kilograms of ozone per cubic meter needed to meet the limit concentration of 0.3 mg/L.

13.34 A raw water contains 40 mg/L ferrous. Calculate the kilograms of dissolved oxygen per cubic meter needed to meet the limit concentration of 0.3 mg/L.

13.35 A raw water containing 3 mg/L of manganese has a pH 4.0. To remove the manganese, the pH needs to be raised to 6.0. The current acidity is 30 mg/L as CaCO3. Calculate the amount of lime needed.

13.36 A raw water containing 3 mg/L of manganese has a pH 4.0. To remove the manganese, the pH needs to be raised to 6.0. The current acidity is 30 mg/L as CaCO3. Calculate the amount of caustic needed.

13.37 A raw water contains 2.5 mg/L Mn. Calculate the solids produced per cubic meter of water treated. The effluent is to contain 0.05 mg/L of manganese and the removal is to be done at the low pH range using chlorine to oxidize the manganous ion.

13.38 A raw water contains 2.5 mg/L Mn. Calculate the solids produced per cubic meter of water treated. The effluent is to contain 0.05 mg/L of manganese and the removal is to be done at the low pH range using dissolved oxygen to oxidize the manganous ion.

13.39 A raw water contains 2.5 mg/L Mn. Calculate the solids produced per cubic meter of water treated. The effluent is to contain 0.05 mg/L of manganese and the removal is to be done at the low pH range using ozone to oxidize the manganous ion. 