What is the largest molarity of generic ion, M*, that will not cause precipitation of a metal sulfite, M2SO3. (Ksp = 1.53 x 108) in a solution that is 8.18 x 10-2 MK2SO3? Report your answer in scientific notation to 3 significant figures. Selected Answer: Correct Answer: 2.29E-6 4.32E-4
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- During titration experiment, you were required to prepare solution for: 2.00M HCl (32% stock solution and density= 1.160 g/ml) The correct calculations to prepare this solution in 100 ml volumetric flask will beChoi is fond of carbonated beverages so he crafted his own soda formulation called “Sodalicious.” Ulan, who is a fellow enthusiast, also made her own formulation which she called “Soda Pop!” to challenge his friend Choi. To know which formulation is better, they sought to determine the carbonic acid content of their soda formulations using titration. In the first part of their experiment, a 0.5 Mlabeled NaOH solution was standardized against 0.350 grams of KHP (MW = 204.22 g/mol) primary standard that is 99.6% pure. The titration required 3.16 mL of the NaOH solution to reach the phenolphthalein endpoint. In the second part of their experiment, Choi and Ulan independently prepared their samples by taking 25.0-mL of their soda sample and diluting it to 30.0 mL. Using the same titrant and indicator, Choi’s “Sodalicious” required 1.39 mL of the standardized titrant to reach the endpoint, while Ulan’s “Soda Pop!” required 0.926 mL of the same titrant to reach the endpoint. A. What is the…Choi is fond of carbonated beverages so he crafted his own soda formulation called “Sodalicious.” Ulan, who is a fellow enthusiast, also made her own formulation which she called “Soda Pop!” to challenge his friend Choi. To know which formulation is better, they sought to determine the carbonic acid content of their soda formulations using titration. In the first part of their experiment, a 0.5 Mlabeled NaOH solution was standardized against 0.350 grams of KHP (MW = 204.22 g/mol) primary standard that is 99.6% pure. The titration required 3.16 mL of the NaOH solution to reach the phenolphthalein endpoint. In the second part of their experiment, Choi and Ulan independently prepared their samples by taking 25.0-mL of their soda sample and diluting it to 30.0 mL. Using the same titrant and indicator, Choi’s “Sodalicious” required 1.39 mL of the standardized titrant to reach the endpoint, while Ulan’s “Soda Pop!” required 0.926 mL of the same titrant to reach the endpoint. D. Calculate…
- In a gravimetric determination of a soluble sulfate the data gathered is presented (see attachment). Calculate the amount of BaCl2 needed fortitration.Q1)a) In the gravimetric analysis the precipitate should be free from impurities. Give the detailed justification for the above statement by identifying impurities. b) It is required to analyse the metal from its ore sample. Manganese (Mn)present in the ore sample was analysed by forming a precipitate of MnSO4. If 2.98 g of ore sample gives 0.19 g of MnSO4. Calculate the percentage of Mn present in the sample.MnO4- can be used in a redox titration to determine the amount of H2C2O4 in an unknown sample. Below is an unbalanced reaction that describes this process: MnO4- + H2C2O4 --> Mn2+ + CO2 25.00 mL of a solution containing an unknown amount of H2C2O4 (MW = 90.03 g/mol) required 18.31 mL of 0.1153 M MnO4- to react completely. Calculate the molarity of the original unknown H2C2O4 solution.NOTE: This is a redox titration, so remember to balance each half reaction and then add them together to arrive at the overall balanced reaction. To help you out, I will tell you that each C in H2C2O4 has a 3+ charge. Also, if your overall balanced reaction doesn't have 8 waters on the right, you have done something incorrectly.
- A solid sample containing some Fe(2+) ion weighs 1.923 grams. It requires 36.44 mL 0.0244 M KMnO4 to titrate Fe in the dissolved sample to a pink end point. Chemical equation: 8H(+) + MnO4(-) + 5Fe(2+) --> Mn(2+) + 4H2O + 5Fe(3+) How many moles MnO4(-) ion are required? How many moles Fe(2+) are there in the sample? How many grams of iron are in the sample? Whats the percentage of Fe in the sample?1.00 grams of table salt was dissolved in 100 mL water and excess AgNO3 reagent was added and yielded 2.3789 grams of precipitate. Calculate the percentage of NaCl in the table salt. Answer must be in 2 significant figures.Write balanced net ionic equations for all reactions in which a precipitate formed. You must show sates and charges for all ions and compounds, (aq), (s) etc. please look at the chart attached. All the boxes with writing had precipate formed. Ex. Mg+2 + CO3-2 ..etc Please provide only typed answer solution no handwritten solution needed and please do it all for instant positive rating
- Prepare 100.00 mL of a solution with the following chemicals; solid FeCl3 6H2O, iron(II) chloride hexahydrate (source of FeCl3) dilute hydrochloric acid in the rack – 3.0 M solid sodium salicylate – 99.7% assay Concentrations: FeCl3: 0.020 M HCl: 0.050 M Salicylate (mg/L): 40.25 PLEASE SHOW HOW TO CALUATE AND WORK. The only equations you will need to use are the equations for molarity and dilutions.When all of the following are mixed together in a beaker, what is the molar concentration of the SCN- ion in the solution just after mixing but before any reaction takes place? 10.00 mL of 2.00 x 10-3 M Fe(NO3)3 4.00 mL of 2.00 x 10-3 M KSCN 4.00 mL of 0.50 M HNO3 answer is between 0.004 and 0.005, please explain how with steps.A solution of 25 mL Na2CO3 is neutralized with 22.4 mL of 0.1065 M HCl. In the another analysis, 50 mL of Na2CO3 solution is added to 25.0 mL of Pb(NO3)2 solution, and after the lead (II) carbonate was filtrated, the excess of Na2CO3 is neutralized with 14.8 mL of the same acid. According to this, calculate the concentration of lead (II) nitrate (331.2 g/mol) as molarity and g/L?