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- Question Content Area Use the following data to calculate the value for each solid. The solubility of CoC2O4 is 2.0*10^-4 mol/L. The solubility Au(OH)3 of is 2.12*10^-12 mol/L.Please help with atleast 3qs as per guidelines. Need correct solution.If 30.0 mL of 1.00 M DNO3 solution is mixed with 20.0 mL of 1.00 M M2CrO4 solution the precipitate X2CrO4 is formed. What species is/are present in solution after the reaction is complete? Note that the precipitate itself is not considered to be in solution. Select all that apply. D+ none of these water CrO42- NO3- M
- Please answer 4 and 5 4. Determine the molar solubility of the M2+ and F- 5. Determine the Ksp value of MF2A stock solution of approximately 7.7x10^-5 molar will be provided in lab. Determine the volumes of each solution needed to prepare 50.00 mL of standard solutions of concentration 0.600x10^-5molar, 1.20x10^-5molar, 2.40x10^-5molar, and 3.00x10^-5molar. Round the calculated volumes to thenearest 0.1mL.The following table gives the concentration of norepinephrine ( mol per gram creatinine) in the urine of healthy volunteers in their early twenties. (show complete solution) follow up question: Is there any evidence that concentration of norepinephrine differs between thesexes?
- Calculate the Molarity (moles per liter) of H2SO4 solution if 40.00 mL of H2SO4 required 42.10 mL of 0.0600 M NaOH to reach a pink phenolphthalein endpoint during a titration. Show work – must have correct number of significant figureYou need to prepare 250. mL250. mL of a 0.400 M0.400 M aqueous solution using a pure solid with a molar mass of 303.3 g/mol303.3 g/mol. Based on your answer to the previous question, what is the value of ?x? ?=40.00 mL of unknown calcium hydroxide solution is titrated with 0.200 M standard nitric acid solution. If 41.60 mL of the standard acid solution is required to reach a phenolphthalein endpoint, what is the molarity of the unknown calcium hydroxide solution? (Hint: write the balanced formula unit equation.)
- The solubility of Ni(OH)2 in a pH = 10.64 solution is___. Ksp Ni(OH)2 = 1.6 × 10-16A solvent of acetic acid (CH3CO2H) is collected consisting of 0.4096 moles. The solute added consist of 0.18744g Ba(OH)2. Assume the change in temperature is 1.0 °C. What is the freezing point depression constant (kf) of the solvent for this example. [CH3CO2H=60.052g/mol] [Ba(OH)2=171.34g/mol] Is the freezing point depression constant calculated in a acetic acid pure? Hint: compare the calculated kf value of acetic acid to the known kf value of acetic (see page 193(93)) in your lab manual. If they’re the same, it’s pure. If they’re not the same, it’s not pure.do both plzzz do not give incomplete solution