
8. A 200 mL sample of water has an initial pH of 10. Thirty millilitres of...
A student is running a titration in the laboratory to determine the alkalinity (Total, bicarbonate and carbonate, hydroxide) of a drinking water sample. The initial pH of the sample is 11.6; 0.02N H2SO4 is used as the titrant; and the sample volume subjected to the titration is 100 mL (0.1L). The results of the titrations were as follows: 18.3 (volume of titrant to drop the pH from 11.6 to 8.3) = 10.0 mL; V4.5 (volume of titrant to drop the...
1a.) From water sample, 10 mg/L HCO3- as CaCO3, 10 mg/L CO3- as CaCO3 and 50 mg/L Ca+ as CaCO3 were measured. pH was near neutral. What is alkalinity? _____ mg/L as CaCO3 1b.) From water sample, 10 mg/L HCO3- as CaCO3, 10 mg/L CO3- as CaCO3 and 50 mg/L Ca+ as CaCO3 were measured. pH was near neutral. What is alkalinity? _____ mg/L as CaCO3 1c.) Calculate Ksp = _____ A2BO3 ->2A++ BO32- Molar concentration of A+ = Molar...
A sample of water at pH 10.5 has 39.0 mg/L of CO32 and 24 mg/L of HCO3 a) Ignoring the contribution of [H] and [OH] to alkalinity, what is the alkalinity as CaCO3? b) Include the contribution of [H] and [OH], find the alkalinity as CaCO3
Alkalinity: The approximate alkalinity of a water sample is 2.21 x 10-2 M at pH=10.33. Determine the concentration of carbonate (CO32-) in M and mg/L as CaCO3. (pKa=10.33). Answer: [CO32-] = 7.37x10-3 M and 737 mg/L as CaCO3 Please show the solution to this problem.
A water sample has a total hardness of 275 mg/L as CaCO3 and a total alkalinity of 320 mg/L as CaCO3. What are the carbonate and non-carbonate hardness (in mg/L as CaCo2) of the water sample? Use the relationship when alkalinity < total hardness, carbonate hardness(mg/L) - alkalinity(mg/L) and when alkalinity >/= total hardness Carbonate hardness(mg/L) -totalk hardness(mg/L) if necessary
A water sample has 5 mg/L of Nitrate, 10 mg/L of Potassium, 60 mg/L of Calcium, and 60 mg/L of Magnesium. If the alkalinity is 394 mg/L of CaCO3, calculate the Total Hardness, Carbonate Hardness, and Noncarbonate Hardness using all polyvalent cations.
Answer units Save Question 7 (10 points) A 100.00 mL sample of hard water is to be titrated with 0.03505 M EDTA solution. A small amount of Mg2+ (that required 1.63 mL of EDTA to titrate as a blank solution) is added to the hard water sample. This sample requires 13.47 mL of EDTA to reach the endpoint. What volume of EDTA is used in titrating the Ca2+ in the hard water? Your Answer units Answer Save
A 11.3-mL sample of an HCl solution has a pH of 2.085. What volume of water must be added to change the pH to 4.170? (in mL)
6. (8) A 50.0 mL sample of hard water containing Ca2 was titrated with 0.0500 M EDTA standard solution at pH 10 and with Eriochrome Black T indicator. The endpoint was reached when 11.35 mL of EDTA was added a) (6) Calculate the concentration of Ca* in the unknown sample in moles per liter (M). b) (2) What is the pCa of the solution?
To determine the Ca^2+ concentration in water sample, a standard EDTA solution of 0.01988 M was used to titrate 25 ml. of the sample solution with the presence of an ammonium buffer (pH 10). If 15.80 ml. of the standard EDTA was used to reach the end point, calculate the molar concentration and the ppm concentration of the unknown Ca^2+ (atomic weight of Ca = 40.08g/mole) solution The amount of 0.2915g of benzoic acid was dissolved in 100 ml. of...