A titration is performed to determine the amount of sulfuric acid, H2SO4, in a 6.66 mL sample taken from car battery. About 50 mL of water is added to the sample, and then it is titrated with 31.52 mL of a standard 0.4643 molar NaOH solution. What is the molar concentration of sulfuric acid in the original sample?

An analytical chemist weighs out 0.170 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1200M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 21.1 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. 0 g mol 0x x10 X S

What is the pH of (3.21x10^-1) M C5H5NHBR? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: х10 Answer

Be sure your answer has the correct number of significant digits.

Will the calculated Molarity of NaOH be too high or too low or unaffected if the following happen: When you answer the question, consider how the situation affects the calculation of molarity of NaOH and moles NaOH, which is calculated from the mass of KHP. For each answer, you must supply a clear explanation for your answer. Often times, students will restate the facts rather than explaining why they chose the answer they chose. a) You add the weighed KHP to a flask containing a 60mL of water rather than 50 mL of water. Explain. Your answer must contain a well-thought-out and clearly written explanation. b) The buret is still wet with water on the inside when you add your NaOH solution. Explain c) The KHP is wet when you weigh it. Explain. d) You titrate past the equivalence point by 0.50mL Answer a-d

An analytical chemist weighs out 0.138 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.0600M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 25.5 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. 0 mol X S 629 OL A

Using mass concentration to find solute mass and solution volume.

Please don't provide handwritten solution ...

Part A Constants I Periodic A 0.5880 g sample of impure magnesium hydroxide is dissolved in 102.0 mL of 0.2044 M HCl solution. The excess acid then needs 19.88 mL of 0.1039 M NaOH for neutralization. Calculate the percent by mass of magnesium hydroxide in the sample, assuming that it is the only substance reacting with the HCl solution. Express your answer using four significant figures. ΜΕ ΑΣΦ Submit Request Answer Provide Feedback LG Backspace F12 1 ? % Delete End Down Next >

Please help me answer questions 1 and 2. (Questions attached below) 1. When you arrive at the lab, 2.0 M H2SO4(aq) and 2.0 M HC2H3O2(aq) will be present. Youwill need to dilute these solutions using beakers and graduated cylinders from your drawerand DI water.i. Calculate the volume of the 2.0 M HC2H3O2(aq) and DI water needed to create 50.0 mLof 1.05 M HC2H3O2(aq).ii. Calculate the volume of the 2.0 M H2SO4(aq) and DI water needed to create 50.0 mL of0.75 M H2SO4(aq). 2. A 48.33-mL sample of 0.150 M NaBr is titrated into 50.00 mL of 0.145 M AgNO3. Bothsolutions had the same initial and final temperatures. The reaction occurred in a calorimeterwith a known heat capacity and produced 1546.03 J of heat.i. Write a balanced equation that is occurring.ii. Determine the theoretical yield of the solid.iii. Calculate the enthalpy of the reaction (kJ/mole of precipitate).