Calculate the hardness in terms of parts per million calcium carbonate (100.0869 g/mol) in a 50.00 mL aliquot of milk sample. The sample was treated with a small amount of ammonia buffer to bring the pH to 10 followed by the addition of 10 drops EBT indicator. The milk sample required 10.00 mL of 8.000 x 10-3 M EDTA for titration. 160 ppm 4 O 80 O 320
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- Na2CO3 served as the primary standard in a titration experiment. Find the molarity of the titrant given the following data in 3 decimal places. Show solutions Primary Standard Used: Na2CO3Formula Mass of 1º standard: 105.99 g/mol% purity of 1º standard: 95% Trial 1 2 3 1º Standard weight, g 0.1005 0.1001 0.0997 Net volume of HCl, mL 9.30 9.00 8.90 Molarity of HCl X1 X2 X3For Ca2+ and Mg2+ determinations in a tap water sample, two 50 mL aliquots were pipetted and placed in different Erlenmeyer flasks. The first of them had the pH adjusted to 12 (Ca2+ titration) and the second to 10 (Ca2+ +Mg2+ titration). The volumes of EDTA (5.07*10-3 mol/L) used in the first and second titrations were 2.40 and 4.80 mL, respectively. Calculate: a) The concentration of Ca2+ in mg/L in the water sampleb) The concentration of Mg2+ in mg/L in the water sampleanswer the following: Let us assume that there is a 0.020 M EDTA titrant solution. Calculate the mass of pure dry CaCO3 standard to use such that the volume of titrant needed to reach the endpoint will be about 35mL if one mole of calcium carbonate reacts with one mole EDTA. Given choices: 0.050 g 0.060 g 0.070 g 0.080 g
- Tony is showing a bacterium having high pH requirement for its growth. He then has to prepare a minimal medium at pH 9. Adding 0.5 ml of the pH indicator to 10 ml of the medium, the solution remained colorless. The pH of the medium was adjusted using 2.25 ml of the 0.05 N titrant. a. What was the pH indicator utilized? b. What is the amount of 1 N titrant needed to adjust 150 ml of minimal medium to pH 9? c.What was the titrant he used?3, Calculate the pH of a solution prepared by mixing 150.0 mL of 0.200 M hydrobromic acid and 150.00 mL of 0.170 M KOH solution. Group of answer choices 1.82 3.25 2.35 2.18 4,Consider the following: HF + NaOH => H2O + NaF 50.00 mL of 0.200 M hydrofluoric acid (Ka=7.2X10-4) was titrated with 35.0 mL of 0.250 M sodium hydroxide. Calculate the pH of the solution at this point. Group of answer choices 5.46 9.39 4.56 3.99A commercial lab received a batch of industrial wastewater samples for analysis. Johnplans to test water hardness of these unknown samples. Prior to complexometric titration,the titrant, EDTA solution needs to be standardized. A 50.00 mL of 5.67 x10-3 M Ca2+standard solution required average of 38.10 mL of unknown EDTA solution to reach itsend point. Based on titration information recorded, work out the correct molarity of EDTAsolution.
- A RbOH solution is titrated four (4) times against potassium hydrogen phthalate (KHP; FW=204.224) samples to the Phenolphthalein endpoint. Using the data below, determine the concentration of the RbOH solution? g of KHP Volume of Base Required 0.5373 g 42.49 mL 0.5856 g 43.88 mL 0.5790 g 48.56 mL 0.5856 g 44.60 mL (Report your answer as "mean +/- std dev") M What is the percent relative standard deviation? % What is the 99% Confidence Interval for the concentration of the solution (population mean)?10.Calculate the pH of the solution prepared by dissolving 0.48 mol of NH3(Kb=1.77x10-5) and 0.750 mol of ammonium chloride in enough water to make 1.00L of buffer solution Group of answer choices A, 5.09 B, 9.05 C, 9.44 D, no correct answer E, 10.1 11,The equivalence point of titrating of the weak base with the strong acid will be observed at Group of answer choices A, pH>7 B, pH<7 C, pH=pKb D, pH>pKb E, pH=7 12,The titration curve of titrating a diprotic acid with a strong base will have two distinct equivalence points Group of answer choices A, if Ka1<<Ka2 B, if Ka1=Ka2 C, always D, in case of ta strong acid E, if Ka1>>Ka2Titration of 50.00 mL of 0.04715 M Na2C2O4 required 39.25 mL of a potassium permanganate solution. 2MnO4- + 5C2O4-2 +16H+ -> 2Mn2+ + 10CO2(g) + 8H2O Calculate the molar concentration of the KMnO4 solution. Pls show step by step. What type of molecules will interfere in this analysis ?
- Indicator A B C pKIndicator 3.8 9.3 5.0 Actual Transition Range (pH) 3.0 to 4.6 3.0 to 4.6 4.4 to 6.2 Consider the titration of 50.00 mL of 0.1000 mol L-1 NH4OH (Kb = 1.75 x 10-5) with 0.1000 mol L-1 HCl.Based on the table above, select the most appropriate indicator to accompany this titration. Justify your choice. What is the theoretical transition range of indicators A, B and C?Use acid-base titration to determine theconcentration of:– A strong acid: HCl 0.100 M NaOH (standardized)•0.100 M HCl0.100 M CH3COOH Phenolphthalein is used for endpoint determination– Changes from colourless to pink as a solution becomes more basic• Only need 2-3 drops per titration• pH range: 8.3-10Titration of 50.00 mL of 0.04715 M Na2C2O4 required 39.25 mL of a potassium permanganate solution.MnO4- + 5H2C2O4 + 6H+ → 2Mn2+ + 10CO2(g) + 8H2OCalculate the molar concentration of the KMnO4 solution.