Calculate the analytical molar concentrations of trichloroacetic acid in an aqueous solution that contains 152.9 mg of trichloroacetic acid,Cl3CCOOH (163.4 g/mol), in 19.3 mL (the acid is 73% ionized in water). Indicate units

A chemistry student is given 1.00 L of a clear aqueous solution at 17 degrees Celsius. He is told an unknown amount of a certain compound X is dissolved in the solution. The student allows the solution to cool to 17 degrees Celsius. The solution remains clear. He then evaporates all of the water under vacuum. A precipitate remains. The student washes, dries and weighs the precipitate. It weighs 0.12 kg. Using only the information above, can you calculate the solubility of X in water at 17° C? If you said yes, calculate it and be sure your answer has a unit symbol and 2 significant digits.

A titration involves adding a reactant of known quantity to a solution of an another reactant while monitoring the equilibrium concentrations. This allows one to determine the concentration of the second reactant. The equation for the reaction of a generic weak acid HA with a strong base is HA(aq) + OH(aq) →A¯(aq) + H₂O (1) A certain weak acid, HA, with a K, value of 5.61 x 10 ", is titrated with NaOH. 6 Part A A solution is made by titrating 9.00 mmol (millimoles) of HA and 2.00 mmol of the strong base. What is the resulting pH? Express the pH numerically to two decimal places. ▸ View Available Hint(s) pH = Submit ▾ Part B pH = IVE] ΑΣΦ Submit A → c More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 66.0 mL ? Express the pH numerically to two decimal places. ▸ View Available Hint(s) IVE ΑΣΦ A + Ċ ? Doowoon Review | Constants | Periodic Table ?

Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq)+NaHCO3(aq)→NaCl(aq)+H2O(l)+CO2(g)  The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 200.mL of a 0.089M HCl solution. What mass of NaHCO3 would she need to ingest to neutralize this much HCl? Be sure your answer has the correct number of significant digits.

KSCN(aq) + Ag+(aq) → AgSCN(aq) + K+(aq)   By calculation she determines the buret delivered: 6.52108 moles of KSCN. The moles of Ag+ which were present in her sample was:

A solution of sodium hydroxide is standardized against potassium hydrogen phthalate (molecular mass = 204.224 g mol-1). From the following data, calculate the molarity of the NaOH solution. The mass of the KHP is 0.7840 g. Before the titration the buret reading was 0.8400 mL and afterwards it was 39.20 mL. A 85.12 mL sample of a solution of sulfuric acid, H2SO4, is neutralized by 59.82 mL of the NaOH solution from the problem above. Calculate the molarity of the sulfuric acid solution.

A chemistry student weighs out 0.0827 g of phosphoric acid (H,PO4), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.0600M NaOH solution. Calculate the volume of NAOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits. mL FEB 19 ... MacBook Air DII 80 888 F10 F7 FB F9 F4 F3 %23 %24

The value of crotonic acid is 2.04 x 10^-5

A pure organic compound has the formula C4H8SOx. A sample of a compound wasdecomposed; the sulfur was converted to sulfate and titrated in a modified version of theadsorption indicator procedure. From the following data, determine the correct formula forthe compound.Given: weight of sample = 12.64 mgBa(ClO4)2 needed for titration = 10.60 mL of 0.0100 M Ba(ClO4)2

A 0.5504-g sample of KHP (potassium hydrogen phthalate, KHC8H4O4; molar mass = 204.22 g/mol) is completely dissolved in enough deionized water to make 50.00 mL of solution. The titration of this solution with a KOH solution requires 20.50 mL of the base (KOH solution) to reach the “end-point”. What is the molar concentration of KOH solution? The reaction occurs as follows:                       KOH(aq)  +  KHC8H4O4(aq)  -->  K2C8H4O4(aq)  +  H2O(l)           (A) 0.2457 M           (B) 0.1315 M           (C) 0.05390 M           (D) 0.03823 M