What is the total mass, in grams, of precipitate that can be produced by mixing 11 g magnesium chloride dissolved in 250. mL of solution and 280. mL of a 0.11 M silve: solution?
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- PLEASE SHOW SOLUTIONS QUESTION NO. 1: A 0.097 N silver nitrate solution of 56.3 ml was used to titrate two samples of sodium lauryl sulfate with 3g and 5g, each respectively. Calculate the %NaCl in the sample, then interpret. Please answer very soon will give rating surelyD. Water Softening 1.For this part of the experiment, watch the video on the link(s) below: https://www.youtube.com/watch?v=jDgSohKVLio Question: Comparison between the relative amount of precipitates for soft vs. hard water.A 60.00-mL sample of a acetic acid is titrated with 0.0361 M NaOH. At the endpoint, it is found that 38.23 mL of titrant was used. What was the concentration of the weak acid?
- 4. About 10 mL of concentrated HCl was transferred to a 1-L bottle and diluted to with water. When this solution was used to titrate a sample of pure sodium carbonate weighing 0.3054 g, it took 35.06 mL to reach the methyl red end point. Calculate the molarity of the HCl solution.An acid sample of unknown concentration is contained in a Erlenmeyer flask. Which technique below would be best suited to analytically determine the number of moles of HCl in the sample? a.) Using a pipette b.) Distillation c.) Using a beaker d.) TitrationShow step by step working of the following problem. How many mL of 0.241 M H2SO4are needed to neutralize a 50.0 mL sample of 0.191 M KOH? (Caution: Don’t you think you would need to balance the equation first ?) H2SO4 + KOH K2SO4 + H2O
- I would really appreciate some help in confirming a value computed in a prelab problem to be used in a lab for analytical chemistry! We're working on redox reactions and are looking at the reaction: Fe2+ + K2Cr2O7 + H+ = Fe3+ + K+ + Cr3+ + H2O The final questions asks, "calculate the amount of unknown sample needed to achieve about a 25.00 mL titration volume of 0.01600 M K2Cr2O7 if the %Fe of the unknown is approximately 8%. Make sure to use the coefficients from the balanced reaction" I have found the balanced equation; however, I was hoping to be able to confirm my values! Thank you in advance!Will a precipitate form when 75.0 mL of 0.0250 M magnesium iodide is mixed with 100.0 mL 0.0130 M lead(II) nitrate? Show how you know with the proper calculations and proper dissociation reactionsPls do fast and i will rate instantly for sure Solution must be in typed form A 25.0 mL volume of 0.0106 M KIO3 is pipetted into a 250-mL Erlenmeyer flask. The solution is titrated to the stoichiometric point with 16.25 mL of a sodium thiosulfate solution. What is the molar concentration of the sodium thiosulfate solution?
- A 0.217 g sample of HgO (molar mass = 217 g/mol) reacts with excess iodide ions according to the reaction show below. Titration of the resulting sample solution requires how many moles of 0.10 M KI to reach the equivalence point? Assume complete reaction. HgO + 4 I- + H2O HgI42- + 2 -OHA solution of 100.0 mL of 0.200 M potassium hydroxide is mixed with a solution of 200.0 mL of 0.150 M nickel (II) sulfate. How many grams of precipitate form?Calculations for Acetate Buffer Solutions Molarity of acetic in acetate buffer (below is the data to answer the answer) Deionized water Acetate Buffer Ammonia Buffer pH of solution 6.62 4.59 9.49 Ph of solution after addition of 1 mL of 0.6 M NaOH 12.41 4.71 9.50 pH of solution after addition of 1 mL of 0.6 M HCl 1.38 3.87 9.24 Preparation of Buffer solutions Mass of sodium acetate in acetate buffer ~ 1.1981 Volume of 3.0 M acetic acid in acetate buffrer ~ 3.81 Mass of ammonium chloride ~ 1.2721 Volume of 5.0 M NH4OH ~ 6.00