1. As the acid solution is titrated the pink color forms where the drop first enters the solution but disappears as the solution is mixed. Explain why this happens. 2. You want to standardize am NaOH solution. A buret containing NaOH solution has an initial volume reading of 0.14 mL. 25.00 mL of a 0.1000 M HCl solution is titrated to an endpoint, which occurs at a final buret reading of 27.16 mL NaOH. What is the molarity of the NaOH titrant?

The answer is not 4.8 x 10^-10 please find the correct answer. Thank you!

A titration process is done by using 0.2M of 20 ml of third analytical group main reagent solution with 0.1 M nitric acid solution if nitric acid is replaced by sulphuric acid of same concentration, then the volume of sulphuric acid equals.... a. Half the volume of nitric acid b. Double the volume of nitric acid c. The volume of nitric acid d. Quarter the volume of nitric acid

A 10.0 mL sample of fruit juice is titrated with 7.55mL of NaOH solution. The molar concentration of the NaOH solution of 0.101M.  A) Calculate the molar concentration of citric acid in the fruit juice. B) Determine the moles of citric acid per serving of the fruit juice. Use 240 mL as the serving size.

An analytical chemist weighs out 0.099g of an unknown monoprotic acid into a 250mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1800M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 10.5mL of NaOH solution.

8. A student conducts an acid-base titration to investigate the change in pH during a reaction between hydrochloric acid and ammonia solution. a. Name a piece of equipment that could be used to provide an accurate measurement of pH during the titration and explain how it would be calibrated. The student transfers 50cm3 of 1.0moldm3 ammonia solution acid into a beaker. During the titration the student adds 50cm3 1.00moldm³ hydrochloric acid from a burette into the beaker and records the pH throughout. b. Sketch the pH curve produced during this titration.

2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)

A student titrates 10.0 mL of 2.0 M formic acid, HCO,H (K.= 1.8 x 10-4), using 1.0 M sodium hydroxide, NaOH. 1. What volume of NaOH solution would be needed to reach the equivalence point? a. 10.0 mL b. 20.0 mL c. 30.0 mL d. 40.0 mL

moles of NaOH moles moles of acid moles Concentration of acid in original sample in M Volume in mL

A 29.00 mLmL sample of an H2SO4H2SO4 solution of unknown concentration is titrated with a 0.1372 MM KOHKOH solution. A volume of 41.22 mLmL of KOHKOH was required to reach the equivalence point. What is the concentration of the unknown H2SO4H2SO4 solution?         Express your answer using four significant figures.