During titration the following data were collected. A 25 mL poretion of an unknown acid soluation was titrated with 1.0 M NaOH. It required 65mL of the base to neutalize the sample. How many moles of acid are present in 3.0 liters of this unknown solution?

Using the table of pH indicators and their respective pKin. Match the best-suited indicator for the following titration scenarios. Note: You do not need to calculate the pH at the equivalence point, an estimation will be sufficient for this question. Indicator Pkin Thymol Blue 1.65 Methyl Red 5.00 Bromothymol 7.30 Blue Phenolphthalein 8.70 0.10 M acetic acid (pKa = 4.74) is titrated with 0.08 M NaOH [ Choose ] 0.10 M HCI is titrated with 0.0993 M NaOH [ Choose ] 0.10 M ammonia (pKb = 4.74) is titrated with 0.12 M HCI [ Choose ]

How do i determine the ml of KOH? (Picture posted) A student used 9.925 x 10-2 mol/L hydrobromic acid to standardize an aqueous solution of potassium hydroxide and obtained the following titration data using phenolphthalein as an indicator:  Concentration of HBr used:                9.925 x 10-2 mol/L Volume of HBr used:                         25.00 mL Indicator:                                            phenolphthalein Endpoint colour change:                     colorless to pale pink

What must be the minimum concentration of hydrocyanic acid in 1.00L buffer solution of a pH 9.8 hydrocyanic acid/sodium cyanide buffer if the pH changes by 0.20 units when 0.032 moles HCI are added? Click here for the table of lonization Constants of Weak Acids. Provide the answer with 3 decimal places. DO NOT use the scientific notation.

I titrate a sample of aqueous sulfuric acid with 14.27mL and 0.117M Potassium hydroxide. Calculate the number of moles of sulfuric acid that were in the sample.

2.74 g of canola oil were titrated with KOH. It required 13.92 mL of 0.0040 M KOH to reach the equivalence point. What is the acid number? Your Answer: Answer units

A 1.00 liter solution contains 0.34 M nitrous acid and 0.44 M potassium nitrite. If 0.110 moles of barium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of barium hydroxide.) VA. The number of moles of HNO2 will decrease. vB. The number of moles of NO2 will remain the same. C. The equilibrium concentration of H30+ will remain the same. D. The pH will decrease. E. The ratio of [HNO2] / [NO2] will decrease.

A technician is adding 50 ml of 1M NaOH to 2000 ml of a 150 mM solution of the carbonic acid buffer that had an initial pH 8.9. They know that at the initial pH the concentration of weak acid was 0.143 M and the concentration of conjugate base was 0.007 M. What pH will the resulting final solution have? Show all details of your working out for each individual mathematical manipulation that you do apply (skipping steps will receive a deduction). The calculation must be presented such that it can be recapitulated by the marker. In each step of your working out use the chemical formulas of the compounds that constitute the weak acid and conjugate base. Provide the final pH to 1 decimal place, make sure to round the result accordingly. State the final answer in a complete sentence.

You measure 0.210 gram of unknown diprotic acid into a beaker. You add distilled water and a chemical indicator.  You slowly add titrant 0.100M NaOH acid solution. Your first equivalence point is reached after 15mL NaOH has been added. The second equivalence point is reached after 30.0mL.  WHat is the molar mass of the unkown diprotic acid?

If you allow your titration to go beyond a faint pink endpoint and it ends up dark pink what effect will that have on your calculated molarity of NaOH? Would you calculate a molarity that is too high to low or no different from the correct molarity