Calculate an unknown concentration of a NaOH solution if 0.224 g of oxalic acid, H2C2O4*2H2O, requires 19.08 mL to complete the titration.  The reaction between H2C2O4*2H2O and NaOH is: H2C2O4 + 2 NaOH --> 2 H2O + Na2C2O4

We have a titration for the titration of 50.0 mL of 0.425 M lactic acid, a monoprotic acid, (Ka = 1.38 x 10^-4) with 0.350 M NaOH.  1. Calculate the exact volume of the NaOH needed (to the correct numbers of sig figs) to reach the equivalence point.  2. Calculate the exact volume of NaOH needed (to the correct numbers of sig figs) to reach the mid point.

The solution started out clear, but when the 12 M HCl was added, lots of the white solid formed. The second round of the eight drops of HCl were added, which produced more white solid taking up most the volume of the test tube. Using the equation and Le Chatelier’s principle, what happened when the HCl was added to the reaction?

5:51 1 .ll LTE Search Question 16 of 20 Submit Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH, with 0.100 M HNO3 after 80.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. 1 2 4 Based on the result of the acid-base reaction, set up the unknown. ICE table in order to determine the H2NNH3*(at H2O(1) =H;O*(aq) H2NNH2(aq + Initial (M) Change (M) Equilibrium (M) RESET 0.100 0.200 0.0333 0.0667 +x -X 0.100 + x 0.100 - x 0.200 + x 0.200 - x 0.0333 + x 0.0333 - x 0.0667 + x 0.0667 - x www

Acetic Acid reacts with sodium hydroxide in the following fashion:CH_3COOH(aq)+NaOH(aq) > H2O(l)+NaC2H3O2(aq) If 3.60mL of vinegar needs 41.0mL of 0.150M NaOH to reach the equivalence point in a titration how many grams of acetic acid are in a 1.50 qt sample of this vinegar? Express your answer using three significant figures

A student performed titration to determine the concentration of citric acid with potassium permanganate solution. The net ionic equation is as follows: 5C6H8O7  + 18MnO4-   + 54H+  → 30CO2  + 47H2O  + 18Mn2+ The concentration of potassium permanganate soluiton is 0.266 M. The volume of lemon juice is 25.00 mL. The titration consumed 17.6  mL of potassium permanganate solution to reach the endpoint. Determine the moles of citric acid in the lemon juice sample.

Each graph below represents a titration involving solutions of two of the following substances: HC2H3O2, HNO3, CH3NH2 and NaOH.   Which graph best represents HC2H3O2 being titrated using NaOH? Which graph best represents HC2H3O2 being titrated using CH3NH2? Which graph best represents HNO3 being titrated using NaOH? Which graph best represents HNO3 being titrated using CH3NH2? Which graph has the lowest pH at the equivalence point? Which graph has the equivalence point pH that is equal to 7?

For humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 0.95 M NaH2PO4 and 0.68 M Na2HPO4. H2PO4-  + H2O ⇌  HPO42-  + H+  pKa= 7.21  (5 marks total) a. From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. (2 marks) b. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places (2 marks) c. If the pH calculated in b. was the blood pH of an actual patient, would you say this patient’s blood pH is in the normal range or are they suffering from alkalosis or acidosis? (1 mark)

This is another titration question. When 35.00 ml of phosphoric acid of unknown concentration is titrated with 1.025 M NaOH, and 18.75 ml of NaOH is required to reach the endpoint, what is the molarity of the phosphoric acid?  The reaction is:  H3PO4 (aq) + 3 NaOH (aq)    →    Na3PO4 (aq) + 3 H2O (l)

A certain weak acid, HAHA, with a KaKaK_a value of 5.61×10−65.61×10−6, is titrated with NaOHNaOH. A solution is made by titrating 8.00 mmolmmol (millimoles) of HAHA and 1.00 mmolmmol of the strong base. What is the resulting pH?   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 47.0 mL ?