Determination of Water Hardness

A 25.00 mL unknown water sample is titrated with a standardized 0.0140 M EDTA solution.  It is determined that 8.54 mL of EDTA is required to reach the end point.  The blank titre was determined to be 1.50 mL.  Determine the concentration of Calcium in the water sample in ppm.  (mwt. of CaCO3 = 100.0892 g/mol).

Determining the Ksp of Calcium Hydroxide: Ca(OH)2 (s) ↔ Ca2+ (aq) + 2OH– (aq) Ksp = [Ca2+][OH–]2 The molarity of the hydrochloric acid used was 0.050 M.15.00 mL of filtered Ca(OH) 2 was measured out for the titration.Calculate the [Ca 2+ ]. Explain, please.  Trial Initial Buret Reading  Endpoint Buret Reading  Endpoint Volume  Equivalence Point Volume  1 80 ml 9.31 pH 12 ml 12.60ml

Given the following information complete the last (blank) data table

Using the two images attached please write one paragraph EXPLAINING THE ANALYSIS Please please please answer as fast as possible Please please try to answer

Determine the concentration of acetic acid and vinegar

A 15.00 mL sample of hard water was titrated with a 0.0150 M EDTA solution. The titration required 26.72 mL of EDTA to reach the end point. What is the total hardness concentration of the water sample in ppm?

5. A water supply company, One Team, found out that their water supply had been contaminated with a sparingly soluble magnesium salt. They requested the help of Magent Analytical Laboratory to identify the magnesium salt. They chose to identify this using Ksp determination after narrowing it down to 2 salts: Salt MgCO3 Mg(OH)2 Theoretical Ksp 3.5 x 10-8 1.8 x 10-11 For the standardization of the HCl titrant, 5.230 mg Na2CO3 (98.9% purity, MW = 105.99 g/mol) required 24.4 mL of the titrant to reach the phenolphthalein endpoint. After isolating and precipitating the magnesium salt A, a portion was dissolved in distilled water in order to make a 250.0-mL saturated solution. The titration of a 50.0-mL aliquot of the saturated solution required 8.20 mL of HCl titrant to reach the phenolphthalein endpoint. Meanwhile, dissolving this magnesium salt in 250.0 mL of 0.0200 M MgCl2 required 1.51 mL of the same HCl titrant to titrate a 100.0-mL solution. a. What is the molarity of the HCl titrant?…

Please write a paragraph of the objective stated using the two images attached below Please please answer as fast as possible thank you

UPLE Using the following data, determine the pH and ionization constant of acetic acid. Procedure and Parameters Initial volume of 0.100 M acetic acid added Volume of distilled water used Conductivity of distilled water Conductivity of the prepared acetic acid Molar conductivity of acetic acid at infinite dilution Results 5.00 mL 50.00 mL 8 μµS.cm-¹ 165 µS.cm-¹ 3.955 x 105 μS.cm-¹-M-¹

Using the two images attached please write one paragraph explaining the analysis Also write another paragraph of the complete method in your own words Please please please answer as fast as possible

You are asked to determine the amounts of calcium ion in a 200 mL water sample using EDTA to titrate the sample. It took 45.5 mL of 0.3 M EDTA to reach endpoint. What is the mass (in grams) of calcium ion in the water sample? Hint: Find out moles of EDTA used to reach endpoint, relate to mol of calcium ion, convert mol of calcium to gram of calcium. The molar mass of Ca is 40.08 g/mol. Round and report your answer to the SECOND decimal place. Numeric value only, no unit.

A 500.0-mg sample of waste ground coffee beans used as fertilizer was digested and analyzed for nitrogen using the Kjeldahl method. After digestion, the distilled ammonia was collected in 100 mL of 0.5500 M boric acid. This solution required 19.60 mL of 0.5880 M HCI for titration to the methyl red end point. Calculate the %N in the fertilizer. Prelim Rxn: NH3 + H3BO3 --> NH4: H2BO3 Titration Rxn: NH : H2BO3 + HCI --> H3BO3 CI-

If a solution of dissolved acid has pH = 2.5 and the pka for the acid chemical is 4.3 and you measure the concentration of the conjugate []-base to be 10mm, what is the concentration of the acid in the solution? pH = pka + logi [HA]

In a hardness of water determination like the one performed in this experiment, it was found that a 25.00-mL sample of water required 12.25mL of 0.0128 M EDTA solution for complete titration. What is the concentration (molarity) of Ca2+ ions in the water sample? What is concentration of CaCO3 (in mg/L) in the water sample? Describe the hardness level of the water using the U.S. government standards.

Concentration sodium thiosulfate solution used: 0.056 mol L-1 ACCURATE TITRATION VOLUME OF SODIUM THIOSULFATE SOLUTION USED Volume titration 1, (ml) Volume titration 2, (ml) Your Group 15.80 15.75 Group 1 16.05 15.70 Group 2 16.30 16.25 ANALYSIS Average volume used, (mL) Standard deviation Number of moles sodium thiosulfate used, (mol) Number of moles calcium iodate in solution, (mol) Volume of calcium iodate used, (mL) Concentration of saturated calcium iodate solution (mol L-¹) Unrounded value 15.9750 0.26220 Rounded value 15.97 0.262 10.0

10.0 pH 8.15, V= 8.6 mL 8.0 pH 6.0 pH= 3.88 D%3D4,3ml. 4.0 2.0 2.0 4.0 6.0 8.0 10.0 Volume (mL) The figure shows the data obtained in the pH titration of a biochemical substance that is a weak acid. Determine the pK, of this compound. exact number, no tolerance

Preparation and Standardization of KMnO4 solution Experimental data Complete the table below. Trial 1 0.2001 g Trial 2 0.2065 g Trial 3 Weight of sodium oxalate (Na2C2O4, MM= 134 g/mol) Titration data 0.2050 g Final reading Initial reading 29.86 mL 0.00 mL 30.66 mL 30.52 mL 0.00 mL 0.00 mL Total vol. of KMNO4 used Computed Molarity of KMNO4 solution Mean Molarity Computed Normality of KMNO4 Mean Normality of KMNO4 solution Reaction Involved: Calculations:

I need help to calculate this data please thanks a lot

If you could help with the below pre-lab questions please. PRELABORATORY ASSIGNMENT Define the term "salt.'  The solubility of AgCl(s) in water is 1.3 x 10-5 M.  Calculate its Ksp.  The solubility of CsF2(s) in water is 2.1 x 10-4 M.  Calculate its Ksp. The of Pb(OH)2 is 4 x 10-15.  Calculate the molar solubility of this compound.

A student performed three KHP titrations in Part 1 in order to standardize their NaOH solution. They reported the following measurements: Mass of KHP + Vial Mass of 'Empty' Vial Final Burette Reading Initial Burette Reading Determination #1 Determination #2 Determination #3 14.1992 g 14.0219 g 14.0982 g 13.3149 g 13.2301 g 13.2779 g 39.21 mL 0.49 mL 35.46 mL 0.86 mL 37.42 mL 1.59 mL How many moles of NaOH did they use in their third titration? Report your answer to the correct number of significant figures and only report the numerical value (no units).

Redox Titration 2 KMnO4 + 5 (COOH)2 + 3 H2SO4 -------> 10 CO2 + 2 MnSO4 + K2SO4 + 8 H2O

Data for titration of 15.00 mL of vinegar with approximately 1.0 M NaOH. Note you must use the exact concentration of the standard NaOH solution to calculate the moles of NaOH. Quantity Еxample Trial 1 Trial 2 Trial 3 M NaOH (exact concentration) 0.992 M 0.953 M 0.953 M 0.953 M V initial buret reading = V, 0.20 mL 1.20 mL 0.52 mL 0.15 mL V final buret reading = V, 12.90 mL 14.22 mL 13.71 mL 13.31 mL %3D Vep = VNAOH added = V; - V, 12.70 mL 13.02 mL 13.19 mL 13.16 mL Vep = VNAOH in L 0.01270 L 0.01302 L 0.01319 L 0.01316 L moles NaOH = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol MNAOH X VNAOH moles AA = 0.0126 mol 0.0124 mol 0.0126 mol 0.0125 mol moles NaOH V sample = V acid 0.0150 L 0.0150 L 0.0150 L 0.0150 L (15.00 mL) (15.00 mL) (15.00 mL) Actual molarity 0.840 M 0.827 M 0.840 M 0.833 M of AA Average molarity for 3 trials => of AA 0.833 M 1. Report the acetic acid (AA) concentration of vinegar in units of molarity (M). 2. Use your average AA concentration to calculate the mass…

An indirect complexation titration with EDTA can be used to determine the concentration of sulfate. A 0.2500-g sample is dissolved in water and added with Ba(NO₃)₂, this precipitated the sulfate present in the sample. The precipitate was filtered and then dissolved in 25.00 mL of 0.02000 M EDTA. The excess EDTA is then titrated against 0.01100 M Mg²⁺, which required 4.25 mL to reach the end point. A. How many mol of EDTA reacted with BaSO₄? B. How many grams of sulfate is present in the sample? C. Which of the following chemical reaction does not happen in the analysis?  a. EDTA + Mg²⁺ ⇌ Mg-EDTA b. SO₄²⁻ + Ba(NO₃)₂ ⇌ BaSO₄ + 2 NO₃⁻ c. BaSO₄ + EDTA ⇌ Ba²⁺ + SO₄-EDTA

Review the list of common titration errors. Determine whether each error would cause the calculation for moles of analyte to be too high, too low, or have no effect.   ANSWER BANK: Too low, No effect OR Too high   adding titrant past the color change of the analyte solutionrecording the molarity of titrant as 0.1 M rather than its actual value of 0.01 Mspilling some analyte out of the flask during the titrationstarting the titration with air bubbles in the buretfilling the buret above the 0.0 mL volume mark

Determining the Ksp of Calcium Hydroxide:  Ca(OH)2 (s) ↔ Ca2+ (aq) + 2OH– (aq) Ksp = [Ca2+][OH–]2 The molarity of the hydrochloric acid used was 0.050 M. 15.00 mLof filtered Ca(OH) 2 was measured out for the titration.Calculate the Ksp for calcium hydroxide. Explain your calculations Trial  Initial Buret Reading  Endpoint Buret Reading  Endpoint Volume  Equivalence Point Volume  1 80ml 9.31 pH 12ml 12.60ml

You collected the following data from a titration experiment using a 0.123M standardized NaOH solution to titrate a 27.36 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Initial Final Vol Delivered |(mL) Burette Burette Reading (mL) Reading (mL) Trial 1 0.56 19.20 ?? Trial 2 0.57 19.7 Trial 3 0.92 19.56 For just Trial 1, determine the amount of NaOH delivered for the titration with appropriate significant digits. Do not include units. Answer:

In the titration of 25.00 mL of a water sample, it took 19.990 mL of 3.480x 10−3 M EDTA solution to reach the endpoint.   Calculate the number of moles of EDTA required to titrate the water sample. (enter your answer with 3 significant figures)   The total hardness is due to one or a combination of Ca2+, Mg2+, and Fe2+ in your sample. It is convenient to express this hardness as though it was entirely due to Ca2+. Making this assumption, determine the number of moles of Ca2+ present in the bottled water sample titrated. (enter your answer with 3 significant figures)   The total hardness is always listed in parts-per-million (ppm) of CaCO3 (or mg CaCO3 / Kg H2O). Since the density of water is 1.0 g/mL, one ppm would be the same as the number of mg of CaCO3 per liter of water. Determine the number of moles of CaCO3 present in the titrated sample of water, assuming that all the Ca2+ combines with CO32−. (enter your answer with 3 significant figures)   Calculate the number of grams of…

A student performed three KHP titrations in Part 1 in order to standardize their NaOH solution. They reported the following measurements: Mass of KHP + Vial Mass of 'Empty' Vial Final Burette Reading Initial Burette Reading Determination #1 16.7538 g 16.2649 g 21.67 mL 0.40 mL Determination #2 14.1709 g 13.5560 g 26.98 mL 0.31 mL Determination #3 15.6625 g 15.0833 g 26.04 mL 0.93 mL How many moles of KHC8H4O4 did they use in their second titration? Report your answer to the correct number of significant figures and only report the numerical value (no units).