(1) Calculate the amount of lime and soda required for softening 9000 litres of water sample containing in ppm, Mg(HCo = 50; CaCl, = 111; MgSO, = 120; CaSO, = 138; NaCi = 480 and Fe-O, = 234, Thelime of 80% and soda of 90% purity was utilized in the process.(i) You are given a task to treat the hard water to produce clear, transparent, and softened water (the residual hardness up to 20 ppm is allowed). As a responsible engineer of the plant, what is your strategy togenerate the water of required softness? Explain

(i)The temporary hardness in water is due to the presence of calcium and magnesium carbonates and…

Answered: ) Calculate the amount of lime and soda…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Mass solute needed to prepare 0.500L of 0.2 M NaCO3 from a solid NaCO3 with a purity of 92.0wt%
You are required to prepare 5 L of a solution containing 1.000 x 103 mol/L of Cu2"(aq). Which of the following procedures would produce an appropriate solution? O Dissolve 0.0636 g of copper metal in nitric acid, add to a 5.000 Lvolumetric flask, dilute to the mark with deionized water and mix well. O Dissolve 1.248 g of CuSO.5H,0(s) in deionized water, add to a 5.000 L volumetric flask, dilute to the mark with deionized water and mix well. Dissolve 0.250 g of CUSO,.5H,O(s) in deionized water, add to a 5.000 L volumetric flask, dilute to the mark with deionized water and mix well.
A 0.1475-M solution of Ba(OH)2 was used to titrate the acetic acid (60.05 g/mol) in a dilute aqueous solution. The following results were obtained. (See attached image)(a) Calculate the mean w/v percentage of acetic acid in the sample.(b) Calculate the standard deviation for the results.(c) Calculate the 90% confidence interval for the mean.(d) (d) At the 90% confidence level, could any of the results be discarded?
A STOCK SOLUTION containing 0.1581 g/L K2CrO4 was prepared.In order to make the CALIBRATION STANDARD, 5 ml of the STOCK was transferredinto a 50ml volumetric flask and then diluted with an appropriate solvent.Calculate:(a) The ppm of K2CrO4 in the CALIBRATION STANDARD.(b) The molarity of K2CrO4 in the CALIBRATION STANDARD. (c) Calculate the molar absorptivity of K2CrO4 (at 371.0 nm). Assume that Beer's Law isobeyed over this concentration range.At 371.0 nm, this CALIBRATION STANDARD in a cell of path length 1.00 cm gave a %T of 59.752.
A solute with a partition coeffcient (K-[S)s/S]h) of 5 is extracted from 20 mL of phase 1 into phase 2. What volume of phase 2 is needed to extract 90% of the solute in one extraction? ( (a) 0.44 mL (b) 12 ml (c) 36 ml. (d) 72 ml
A sample containing iron is approximately 99.0% w/w Fe. Using ammonia, iron is precipitated as Fe (OH)3 which is ignited to Fe203. (a) What is the gravimetric factor for analyte Fe (AW=55.85 g/mol) and precipitate Fe203 (FW=159.69 g/mol)? (b) What mass of sample is needed to ensure that the Fe203 precipitate would weigh at least 1.00 g?
SO4 -two content in 7689mL of a water sample was precipitated as Na2SO4. The precipitated was filtered, washed and calcined in an empty crucible with a mass of 27.0234g. The mass of the crucible plus Na2SO4 (142g/mol) was 27.7708g. Calculate the %m/v of Na (23g/mol) and the concentration of Na in the sample in ppm.
KMnO4 and Na2C2O4 solutions were used in the reactions that took place in a back titration to determine the amount of H2O2 in a sample. Calculate the concentration of H2O2 in the sample (w / v) as% by making appropriate assumptions for the volumes and normality of all these solutions.
Predict three (3) correct apparatus used for the procedures experiment run by a chemist below. Determination of phosphorus in plant food will produced magnesium ammonium phosphate, MgNH4PO4.6H2O, precipitate. The precipitate was kept in a crucible and dry at 130 °C for 2 hours. Then, the precipitate was cooled for 15 minutes in a condition of low moisture atmosphere. The precipitate is weighed until constant weight is obtained.
4.0g of potassium hydrogen tartrate was added to 300mL distilled water. The temperature of the solution is 23.1C. The liquid was filtered and 50mL of the filtered solution was transferred to 250mL beaker, two drops of phenolpthalein was added to the 250mL beaker. The concentration of NaOH is 1.0 M that is filled in the 2mL graduate pipette, single drops of NaOH was added to the 250mL beaker until the solution turns pink and the potassium hydrogen tartrate reach the endpoint. The datd of four trials was collected. Please answer the following questions 4) calculate ksp for potassium hydrogen tartrate for each trial and average ksp for thr experiment 5) calculate the percent error in you value of ksp using reference that is found as the theoretical value. 6) why was the temperature of the saturated solution recorded?
4.0g of potassium hydrogen tartrate was added to 300mL distilled water. The temperature of the solution is 23.1C. The liquid was filtered and 50mL of the filtered solution was transferred to 250mL beaker, two drops of phenolpthalein was added to the 250mL beaker. The concentration of NaOH is 1.0 M that is filled in the 2mL graduate pipette, single drops of NaOH was added to the 250mL beaker until the solution turns pink and the potassium hydrogen tartrate reach the endpoint. The datd of four trials was collected. Please answer the following questions 1) calculate the total volume and moles of NaOH required to reach the endpoint for each trial. 2) calculate the molar solubility of potassium hydrogen tartate ( in mol/L) for each trial. 3) calculate the average molar solubility of potassium hydrogen tartate for the four trials. What is the average solubility of potassium hydrogen tartrate in g/L? 4) calculate ksp for potassium hydrogen tartrate for each trial and average ksp for thr…
alarity and Normality. 2- Calculate the weight of solute in grams for each of the followings solutions: (a) 43.5 mL of O.175 N Hg(NO;)2 (b) 10 mL of 0.03 N KI if the reaction product is Agl (c) 5 litres of 0.25 N K2CO7 in acidic medium. nolarity, normality and part per million

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