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A 50.00-mL sample of a white dinner wine required 24.57 mL of 0.03291 M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated).

5:50 1 Search Question 5 of 20 Submit Determine the mass of solid NaCH;COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH3COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH-COОH is 1.8 х 10-5. 1 2 Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH3COOH+ H20(1) =H;O*(aq) +CH3COO-(a Initial (M) Change (M) Equilibrium (M) 5 RESET 0.200 5.00 -5.00 1.0 x 10-9 -1.0 × 10-9 1.0 x 10-5 -1.0 x 10-5 1.8 x 10-5 -1.8 x 10-5 х+ 5.00 x - 5.00 x + 1.0 × 10-9 х - 1.0 х 10-9 1.0 x 10-5 x - 1.0 × 10-5 x + 1.8 × 10-5 х - 1.8 х 10-5

Limestone consists mainly of the mineral calcite, CaCO3.  The carbonate content of 0.5143 g of powdered limestone was measured by suspending the powder in water, adding 10.00 mL of 1.396 M HCl, and heating to dissolve the solid and expel the CO2: CaCO3(s)  +  2H+  ⟶⟶ Ca2+  +  CO2↑↑ +  H2O The excess acid requied 39.96 mL of 0.1004 M NaOH for complete titration: OH-   +   H+  ⟶⟶ H2O Find the weight percent of calcite in the limestone.

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You are studying a clear solution and you added the pH indicator methyl violet. The colour range of the indicator methyl violet in a clear solution when changing from acidic to basic is yellow (pH 0) to blue purple (pH 1) to violet (pH 2). You initial pH of the solution when tested with a pH meter is O.2. You are going to add 250 drops of 0.1 M HCI. Please select the most appropriate answers to the following two questions. What is the initial colour of the solution at pH 0.2? What is the colour of the solution and what will the pH be after the addition of the HCI? Select 2 correct answer(s) The colour of the solution after the addition of HCI will be clear and the pH will be less than 0.2. The colour of the solution after the addition of HCI will be violet and the pH will be higher than 0.2.

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A chemist titrates a 25.0 mL sample of 0.239 M benzoic acid (C6H5COOH) against a 0.100 M solution of NaOH.The overall reaction is shown by the equation below: C6​H5​COOH(aq)+NaOH(aq)C6​H5​COONa(aq)+H2​O(l) The Ka value for benzoic acid is 6.28 × 10–5. Calculate the pH at the start of the titration, before any NaOH has been added. Give your answer correctly to two places after the decimal.

A 44.6 mL of 0.103 M HCI is added to an antacid sample. The solution is titrated to a bromophenol blue endpoint using 19.8 mL of 0.0998M  NaOH. How many moles and how many grams of the base are in the antacid sample? Assume the active ingredient is MgCO3.  Moles of NaOH? Moles of HCl? Moles of MgCO3? Mass of MgCO3?

Determine the differences in pH when a strong base is used to titrate a strong acid and a weak acid. Consider the following reactions: HC1 (ад) + NaOH (aq) → NaCl + H2O a (ад) HC;H;O2 (aq) + NaOH → NaCH;O2 (ag) + H2O ) (аq) Experiment 1: 0.2773 M NaOH is used to titrate 10.00 mL of 0.7198 M HC1 Experiment 2: 0.2773 M NaOH is used to titrate 10.00 mL of 0.7198 M HC:H;O2 (K. = 1.75 x 10*) Because the volumes and concentrations are the same for both titrations, the volume of titrant required to reach the equivalence point is also the same: 25.96 mL of NaOH. Calculate the following: 1. The pH of both acids before any base has been added (initial pH). 2. The pH at the equivalence point for the HCH;O2 + NaOH titration. 3. The pH when 25.00 mL has been added in the HCl + NaOH titration 4. The pH when 8.00 mL has been added in the HC:H;O2 + NaOH titration,

Similar to acetic acid, propionic acid (CH3CH2COOH) is a weak acid (HA), which inhibits the growth of mold and some bacteria and also used to make pesticides and pharmaceuticals. Suppose 10.00-mL of 0.8000 M propionic acid (CH3CH2COOH), is titrated with 0.2000M NaOH. Ka for propionic acid is 1.4 x 10-5 . What is the pH after addition of 30.00 mL of NaOH to the propionic acid solution?

You have a 18 mL sample of acetylcholine (a neurotransmitter) with an unknown concentration and a pH of 7.82. You incubate this sample with the enzyme acetylcholinesterase to convert all of the acetylcholine to choline and acetic acid. The acetic acid dissociates to yield acetate and hydrogen ions. At the end of the incubation period, you measure the pH again and find that it has decreased to 5.66. Assuming there was no buffer in the assay mixture, determine the number of nanomoles of acetylcholine in the original 18 mL sample. Tip: your answer should have two significant digits! Only the mantissa (the digits to the right of the decimal) are significant when you raise a decimal number to a power. CH,—C−O−CH,—CH,—*N—CH, Acetylcholine CH 3 acetycholine in original sample: CH3 H₂O CH3 HO–CH,—CH,—*N–CH, + CH, Choline CH3 CH, T Acetate O + H+ nmol