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Q: ) What four attributes must one have for a primary standard? b) State which chemical used in this…
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Q: if the KSP of AgCl is 1.8 x 10^-10, how many grams of AgCl can be dissolved in 500mL of H20
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Q: Calculate the solubility of Ba(IO3)2 in water (Ks = 1.57×10-9).
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- What is the importance of non-aqueous titrations in pharmaceutical analysis?Why Mg2+ is precipitated during lime-soda softening as Mg(OH)2(s) rather than MgCO3(s)? Please urgently3 possible errors that can lead to a difference between the theoretical concentration and actual concentration of a standard solution
- (c) What is a standard solution? What piece of glassware is used to prepare a standard solution and describe how a standard solution of sodium carbonate may be prepared in the laboratory?3. How would you prepare 50.0-ml portions of standard solutions that are 0.00500 M, 0.00200 M, and 0.00100 M in Na" from the 0.0100 M Na" solution?1. A silver nitrate solution contains 14.77 g of primary standard AgNO3 in 1.00 L. What volume of this solution will be needed to react with a) 0.2631 g of NaCl? b) 0.1799 g of Na CrO4? c) 64.13 mg of NazAsO4?
- In this experiment, your goal is to determine the amount of lead present in a water sample and, if lead is present, to determine whether the level of contamination is potentially dangerous. Preliminary preparation of the sample has resulted in a solid of unknown composition. This solid contains lead (Pb 2+ ) in the form of a water soluble salt and gravimetric analysis will be used to determine the amount of lead present. Step 1. Preparation of precipitating agents : Dissolve a predetermine amount of sodium sulfate in distilled water to produce 100mL with a concentration of 0.175M. Transfer the solution in the burette.Step 2. Obtain 3 10-mL sample of wastewater which contains lead in an erlenmeyer flask.Step 3. Dilute the 10 ml sample with water to 100mL.Step 4. Add an excess amount of sodium sulfate to achieved complete precipitation.Step 5. Filter the solution using a pre-weighed filter paper.Step 6. Collect the precipitates in filter paper and dry in an oven at 105 o C for 3 hrs or…1. The Ksp of Ca3(PO4)2 is 1.3 × 10−26. Estimate the solubility of this salt in units of g. L−12. If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 2.1? Explain you answer in a short sentence. Please only answer 2nd Question1. The Ksp of Ca3(PO4)2 is 1.3 × 10−26. Estimate the solubility of this salt in units of g. L−12. If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 2.1? Explain you answer in a short sentence.
- The Ksp of Cu3 (PO4), is 1.00 × 10-37. Estimate the solubility of this salt in units of g. L-1. You must show any reaction equation(s) that you may think are necessary. If a sample of solid Cu3 (PO4)2 is stirred into exactly one litre of a 0.550M solution of K3PO4 , how will the solubility of the salt compare with the answer that you have obtained in question 2.1? Explain you answer in a short sentence.1. A sample of pure sodium oxalate, Na2C2O4 , weighing 0.2856 g is dissolved in water, sulfuric acid is added, and the solution titrated at 70°C , requiring 45.12 mL of a KMNO4 solution. The end point is overrun and back-titration is carried out with 1.74 mL of a 0.1032 N solution of oxalic acid. Calculate the normality of the KMNO4 solution. Hint: A redox reaction is involed between oxalate and permanganate. Look at the changes in oxidation state by determining the balanced redox reaction: 5C20,2 + + 2MN2+ 2 Mn04 + 10H* → 10CO2 + 8H20It's your turn.... 1. What volume of 4.25 M C6H12O6 is needed to get 205.0 grams of glucose? 2. How many moles of solute are in 250 mL of 2.0 M CaCl₂? How many grams of calcium chloride are present in the solution? ● 3. Calculate the molarity of 0.007 mol of Li₂CO3 in 10.0 mL of solution.