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Q: Calculations Titration 1 Titration 2 Titration 3 Moles of KHP Moles of NaOH…
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Q: 1. 35.0 mL 0.175 M HBr sample is titrated with 0.200 M KOH. a) Initial pH
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Q: tration. e titration
A: “Since you have posted a question with multiple sub-parts, we will solve the first three subparts…
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- (1) Careless Carlie weighed her KHP sample, but forgot to bring her report sheet along, so she recorded the mass of KHP on a paper towel. During her titration, which required 18.46 mL of base, she spilled some base on her hands. She remembered to wash her hands, but forgot about the data on the towel, and used it to dry her hands. When she went to calculate the molarity of the base, Carlie discovered that she didn’t have the mass of her KHP. Her kindhearted instructor told Carlie that her base was 0.2987 M. Calculate the mass of Carlie’s KHP sample. Show calculations (2) What mass of solid NaOH would be needed to make 645 mL of Carlie’s NaOH solution? Show calculations.2-1: Which of the following mixed compounds could be the best to be separated by extraction? NH . OH OCH₂ ONaQ4 | What is the purpose of conducting the recrystalization process of the product ?
- Part A) A 10.0 mL sample of 0.250 mol/L NiF2(aq) is mixed with 20.0 mL of 0.0900 mol/L NaOH(aq) and then diluted to a final volume of 100. mL.Calculate the concentration of Ni2+ ions in the 100 mL mixture before the reaction starts. Express your answer to three significant figures.ksp: 5.48e-1630jud to 28AM basu mw 5. Sodium carbonate is a reagent that may be used to standardize acids in the same way that you have used KHP in this experiment. In such a standardization it was found that a 0.498-g sample of sodium carbon- ate required 23.5 mL of a sulfuric acid solution to reach the end point for the reaction.A (aq) + ...B(aq) C(s) + D (aq) ... .. Experimental | Volume of B/ mL Mass of Run precipitate/g 1 1.2 5.40 2 1.4 7.24 1.6 9.02 4 1.8 9.90 2.0 10.86 6. 2.2 10.90 7 2.4 10.88 8 2.6 10.84 9. 2.8 10.86 A series of experiment was performed to determine the mole ratio of a given reaction. 1 mL of 1 Molar A added to nine beakers, then the increasing amount of 1 Molar B added to these beakers. Volume of B and mass of precipitate of C are given in the table below. Find the mole ratios through plotting a graph.
- ENB Assume the densities of all solutions are 1.0 g/ml and their specific heat capacities 4.184 J/g. Experime The enthalpy change of neutralization Part I 3 NH4OH(aq) + HCl(aq)- NH4CI(aq) + H2O(E) 2.1 Equation of reaction: 2.0 M HCI 2.0 M NH.OH Volume Number of moles 0.05 25 ml 25 ml 0.05 Temperature 15 °C 15 °C eaction Initial Temperature,T Final Temperature, T Change in temperature, AT 15 °C 16.5 °C 1.5 °C Calculation of q- in J (q- = - qsa) 2.2 What is the enthalpy change (AH) in kJ.mol, when 1 mol of acid is 2.3 neutralized?Report sheet for Titration of vinegar Part I: Standardization of the NaOH solution with KHP Trial 1 Trial 2 Trial 3 Mass of Erlenmeyer flask + KHP (g) 78.34 78.27 78.01 Mass of empty flask (g) 77.12 77.12 77.12 Mass of KHP (g) 1.22 1.15 0.89 Final buret reading (mL) 31.35 30.53 27.71 Initial buret reading (mL) 16.35 15.78 14.20 Vol NaOH solution delivered (mL)…Complete the following reaction ia' T-Fe/HCI / AICI Br Br COOH NO,
- Titration of 0.1756 grams primary standard sodium oxalate (134.00 g/mol) dissolved in 50 mL water with 5 mL concentrated sulfuric acid required 32.1 mL of a potassium permanganate solution. redox method used?Which served as the oxidizing agent? Which served as the reducing agent?What is the total number of electrons involved in the redox reaction?What can be used as an indicator for the titration?What is the molar concentration of the titrant?Do you always have to use a primary standard in the standardization of titrant? Why or why not?7-3: Analysis of a Ferrous Chloride Sample Titrations provide a method of quantitatively measuring the concentration of an unknown solution. This is done by delivering a titrant of known concentration into an analyte of known volume. (The concentration of an unknown titrant can also be determined by titration with an analyte of known concentration and volume.) In oxidation-reduction (redox) titrations, the voltage resulting from the mixture of an oxidant and reductant can be measured as the titration proceeds. The equivalence point of the titration, or the point where the analyte has been completely consumed by the titrant, is identified by the point where the voltage changes rapidly over a small volume of titrant delivered. In this assignment, you will determine the mass % of an unknown sample of ferrous chloride (FeCl2) by titrating it with a KMNO4 solution of known concentration. Start Virtual ChemLab, select Electrochemistry, and then select Analysis of a Ferrous Chloride Sample…