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

13.07 ml of an Unknown Acid titrated with 24.03 ml of a Base standardized to 0.10000M. What is the concentration of the unknown acid? Assume the acid and base react in a 1:1 molar ratio.

A 25.00 mL sample of acetic acid (CH3COOH) is titrated to the equivalence using 31.08 mL of 0.1978 M NaOH. What is the balanced neutralization chemical reaction? What is the molarity of the acetic acid in the original sample?

The flask contains 10.0 mL10.0 mL of HClHCl and a few drops of phenolphthalein indicator. The buret contains 0.110 M NaOH.0.110 M NaOH. It requires 31.4 mL31.4 mL of the NaOHNaOH solution to reach the end point of the titration. What is the initial concentration of HClHCl?

You have been provided with a 2.08 x 10-2 L  sample of lithium hydroxide (LiOH) of unknown concentration. You perform a titration with 2.19 M nitric acid (HNO3), and find that 24.6 mL are required to reach the equivalence point (as determined using a coloured indicator). What is the concentration of the lithium hydroxide solution in mol L-1?

55.0 mL of 1.20 M H2SO4 is added to a 39.5 mL of 2.00 M LiOH. The balanced chemical equation for the reaction is: H2SO4 (aq) + 2LiOH (aq) --> Li2SO4 (aq) + 2H2O (l)  What kind of reaction is this? If a phenolphthalein indicator was included in the reaction flask, what color will it be after the 55.0 mL of 1.20 M H2SO4 and 39.5 mL of 2.00 M LiOH have reacted? Clear or pink? Explain your answer and include any relevant calculations.

A solution of oxalic acid dihydrate (H₂C₂O₄･2H₂O) with a known concentration of 0.400 M H₂C₂O₄･2H₂O is titrated with a 0.333 M NaO solution. How many L NaOH are required to reach the second equivalence point with a starting volume of 65.0 mL H₂C₂O₄･2H₂O, according to the following balanced chemical equation:   H₂C₂O₄･2H₂O + 2NaOH → Na₂C₂O₄ + 4H₂O

The calcium in a 200 mL sample of water sample was determined by precipitating the cation as CaC2O4. The precipitate was filtered, washed and ignited in a crucible with an empty mass of 26.6002 g. The mass of the crucible plus Cao (56.077 g/mol) was 26.7134 g. Calculate the Molarity of Ca. a. 0.005 M O b. 0.040 M O c. 0.100 M O d. 0.080 M O e. 0.010 M

a student weights out 1.118 g of impure KHP, dissolves the sample in deionized water and titrates it with 0.1001 M NaOH solution. If the titration requires 2710 mL of the NaOH solution, and non of the impurities react with NaOH, what is the percent KHP in the sample?

Chaya the chemistry student carries out a titration by adding an aqueous solution of NaOH to an aqueous solution of the weak acid HY. The images below represent the solutions formed at various points during this titration. (Na+ and H₂O are omitted for clarity.) HY OY &H30+ О ОН A B C Select the image corresponding to each of the following points in Chaya's titration. Before adding any NaOH : -- + Partway to the equivalence point: -- At the equivalence point : -- After the equivalence point: [ → D E y selecting h menu.