For each part of this question, consider the following scenario: You need to make a stock solution of Mg(HC03)2 with a concentration of 5.50 M. You have a 750.0 mL volumetric flask available to make this stock solution in. You are then tasked with using this stock solution to prepare a sample for use in an experiment. The experimental sample should have a final volume of 5.00 mL and a concentration of 0.150 M Mg(HCO3)2. a) What is the molar mass of Mg(HCO3)2? b) How many moles of the solute would be needed to create the stock solution using the volumetric flask available? c) How many grams of the solute should be added to the volumetric flask to create the stock solution? d) What volume, in mL, of the stock solution should be used to prepare the experimental solution through dilution?
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- Please answer this NEATLY, COMPLETELY, and CORRECTLY for an UPVOTE. Ni(NO3)2From the stock solution (1.0 M), determine the volume needed to prepare 0.00, 0.04, 0.08, 0.12 and 0.16 M Ni(NO3)2 solution in 50 mL volumetric flask. Obtain the calculated amounts, place in corresponding volumetric flasks and dilute to mark.Sample: Saline 0.900% (m/v), in sodium chloride (NaCl). Data: M.A. (g/mol): Na = 22.9898; K = 39.0983; Cr=51.9961; Ag = 107.8682; Cl = 35.453; N=14.0067; O = 15.9994. Material available in the laboratory's warehouse: Reagents: distilled water; standardized solution of silver nitrate (AgNO₃), at a concentration of 0.09980 mols/L; Potassium chromate solution (K₂CrO₄) 1%; ammoniacal ferric alum solution [Fe(NH₄)(SO₄)₂] and; nitrobenzene (or cooking oil, alternatively); 0.1000 mols/L potassium thiocyanate (KSCN) standard solution. Glassware: beakers of all sizes available on the market; 50, 100, 150, 200 and 250 ml Erlenmeyers; 10.00 and 25.00 mL volumetric pipettes; 15.00 mL burette; 30.00, 50.00 and 100.00 mL volumetric flasks Calculate the molarity of saline, in terms of the NaCl concentration (concentration in mols/L). (a) 0.900 mols/L (b) 5.84 mols/L (c) 0.154 mols/L (d) 0.0154 mols/LTwenty vitamin C tablets (total mass = 6.3561 g) were powdered and 0.3181 g dissolved in dilute sulphuric acid. This solution was then titrated with 0.0973 M ammonium cerium (IV) sulphate and 23.24 mL required to reach the end-point. Given that ammonium cerium(IV) sulphate reacts with ascorbic acid in a 2:1 ratio, calculate the mass of ascorbic acid (in mg) per average tablet. Mr (Ascorbic acid, C6H8O6) = 176.12
- In an impure sample of table salt that weighed 0.8421 g when dissolved in water and treated with excess AgN03 formed 2.044 g of AgCl. Listing the percentage of NaCl is in the impure sample. What is the list of three sources of error in this experiment?Q. If we are asked to use the recorded Wright of copper(II)sulfate pentahydrate to calculate the exact concentration of of an experimentally recorded copper II sulfate in volumetric flask, do we multiply the grams of copper II sulfate by the molar mass to get the molarity of the copper? Then, do we use the dilution formula to get the concentration. The recorded mass was 2.493 g for 50ml of copper II sulfate stock solution.When mixing sodium chlorate solution (volume 1.0L, density 1.1614 g/ml, mass fraction 22%) with hydrochloric acid( 2L, density 1.0980 g/ml, mass fraction 20%) an antiseptic substance was released. Write and balance the Mentioned reaction and name this anticipatic substance.
- How many milliliters of a stock solution of 7.00 MM HNO3HNO3 would you have to use to prepare 0.170 LL of 0.550 MM HNO3HNO3? V = Part B If you dilute 16.0 mLmL of the stock solution to a final volume of 0.350 LL , what will be the concentration of the diluted solution? MM =ou are asked to weigh 2 g of lithium and add it to 1500 ml of distilled water +2drops of indicator, knowing that the density of water is 1 at room temperaturewhile conducting this experiment. first, Determine the amounts of the product; (LiOH) After knowing the amount of LiOH, you need to dilute to prepare 0.25 M of LiOH in a 3000 ml solution. Show your calculation and units. Knowing that the initial volume that you used was 1500 ml Use this equation to calculate ( CLiOH x VLiOH) before dilution = (CLiOH x VLiOH) after dilutionThe ingredients in herbicides and pesticides must be carefully monitored. Arsenic in a pesticide sample was precipitated as MgNH4AsO4 (molar mass = 181.25 g/mol). This was heated to form the more stable Mg2As2O7 (molar mass = 310.45 g/mol). Based on the following data, what is the numeric value of the gravimetric factor for the sample?
- How many milligrams of MgI2 must be added to 275.0 mL of 0.0788 M KI to produce a solution with [I−] = 0.1000 M?Describe the preparation of the following solution attached as an image below. P.S. This is not an incomplete question.Twenty tablets (labelled 300 mg aspirin per tablet) had a total mass of 6.9117 g. The tablets were powdered and 0.5423 g of powder was added to 30.0 mL 0.494 M sodium hydroxide solution and the mixture boiled gently for 10 minutes. The excess alkali in the cooled solution was titrated with 0.475 M hydrochloric acid solution and 20.25 mL required for neutralization. Given that aspirin (C9H8O4) and NaOH react in a 1:2 ratio calculate the percentage of aspirin as compared to the labelled claim. Aspirin Mr(C9H8O4) = 180.2