In a titration, 20.0 g of oxalic acid dihydrate was dissolved in a flask and neutralized with 31.2 mL of NaOH. Determine the molarity of the NaOH. 2NaOH(aq) + H2C2O4 ⋅ 2H2O(s) --> Na2C2O4(aq) + 4H2O(l)

A 15.00 mL sample of barium hydroxide requires 23.55 mL of 0.2550 M hydrochloric acid to reach the titration end point. Calculate the concentration of the barium hydroxide solution. 2HCl(aq) + Ba(OH)2(aq) --> BaCl2(aq) + 2H2O(l)

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.

Write a balanced chemical equation for the titration of an aqueous sample of NaHCO3 with HNO3. Be sure to include all states of matter. X x, Не (aq), Na,CO3(ag) + HNO3(aq) NaHCO, (aq) + NaNO, (aq)

ion The following table shows data from the titration of four 25.0 mL samples of a perchloric acid solution, HCIO4(aq), using a 0.225 mol/L sodium hydroxide standard solution. Bromothymol blue is used as an indicator to detect when the endpoint is reached. Titration of 25.0 mL of HCIO4 with 0.225 mol/L NaOH(aq) final burette reading (mL) initial burette reading (mL) volume of NaOH(aq) added (mL) colour at endpoint Trial 1 Use the data in the table below to answer the next two questions. Trial 2 Trial 3 Trial 4 Trial mL . . . mL mL 1 mL 19.9 0.4 2 Using the chart above, provide the volume of NaOH added for each of the trials. 38.8 3 19.3 19.9 0.2 4 38.4 19.3 blue green green green DELL

A chemistry student weighs out 0.315g of ascorbic acid H2C6H6O6 , a diprotic acid, into a 250.mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.0700M 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.

What is the pH of a buffer solution if you have 250 ml of a 1.56M Acetic Acid and you added 26.56 grams of sodium acetate (NaCH3CO2)? What is the new pH if you now add 1gram of NaOH to the buffer solution?

45.02 mL of a saturated solution of iron (III) hydroxide are titrated with 0.253 M HCl.  If 3.36 mL of the acid are required, what is Ksp for iron (III) hydroxide? Iron (III) hydroxide reacts with HCl according to the following balanced equation: Fe(OH)3(aq)  +   3HCl(aq)  →   FeCl3(aq)  +  3H2O(l)

Consider a buffer solution that consists of two separate components: the weak acid, CH3COOH(aq), and its conjugate base, CH3COO¯ (aq)  (added as NaCH3COO).   Which component will react with H+(aq) from a strong acid? Write the net ionic equation for the reaction that occurs when H+(aq) is added to the buffered solution.   Which component will react with OH-(aq) from a strong base? Write the net ionic                  equation for the reaction that occurs when OH-(aq) is added to the buffered solution.

20. Consider the following hypothetical acid-base titration where A represents the acid and B represents the base. The products of this reaction are salt and water. Assume the equation is balanced as written. 3A + 2B --> salt + water (OR 3 A + 2 B right arrow salt + water) Two burets are setup with one containing acid, A, and the other containing base, B. The initial volume of buret A is 1.32 mL and the initial volume of buret B is 1.14 mL. Acid from buret A is added to a flask until the final volume of buret A is 12.10 mL. Base from buret B is added to the flask until the titration reaches the endpoint. The final volume of buret B reads 24.96 mL. Calculate the molarity of the acid, A, if the base has a molarity of 1.213 molar. You may want to create a data table to help you organize your work. Do not type units with your answer.