0.5 gr of a diprotic acid is dissolved in water and titrated with 10 ml 1 M KOH to phenolphthalein end point. What is the molar mass of the acid? ½ H2A (aq) + KOH (aq) --> ½ K2A (aq) + H2O () Molar mass of KOH: 56 gr/mol O a 100 gr/mol O b. 200 gr/mol O. 50 gr/mol O d. 150 gr/mol
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- A 20.00 mL aliquot of lactic acid solution (HCH3H5O3) was titrated with 0.0980 M KOH(aq) using both an indicator and a pH meter. Ka (HCH3H5O3), is 1.38 x10-4. A total of 28.64 mL of 0.0980 M KOH(aq) was required to reach the equivalence point 1. Calculate the molarity of the lactic acid solution. 2. Calculate the pH of the lactic acid solution 3. Calculate the pH and [CH3H5O3-] at the half-equivalence point. 4. Calculate the pH at the equivalence point of the titration. 5. Suggest an appropriate indicator for titration. 6. Calculate the pH of the solution after 10.00 mL of 0.0980 M NaOH(aq) was addedApproximately 6 mL of conc. perchloric acid ( 72% ) was transferred to a bottle and diluted with about 1 liter of water. A sample containing 251.5 mg of primary standard Na2B4O7.10H2O (Fwt= 382g/mol) required 27.41 mL of the HClO4 solution to reach the methyl red end point. What is the molar concentration of the HClO4 solution? Na2B4O7.10H2O + HClO4 ------------> NaClO4 H2B4O7.10H2OWhat is the mass of aectylsaliyclic acid (HC9H7O4, MW = 180.154 g/mol) from an aspirin tablets by titrating with NaOH. One tablet is dissolved in 25 mL of 50% ethanol solution. The resulting solution needed 13.41 mL of 0.2069 standardized NaOH titrant in order to achieve the phenolphthalein endpoint. What is the mg of aectylsaliyclic acid in the asiprin tablet?
- 50 mL sample solution containing Na2CO3 and NaOH is titrated with 0.2 M HCl solution. In the presence of phenolphthalein indicator, the acid consumption is 15 mL. Then, the titration is continued by adding bromocresol green indicator, and in the presence of this indicator, the acid consumption is 10 mL. Accordingly, which of the following is the amount of Na2CO3 (in grams) in the sample? (NaOH: 40 g / mol; NazCO3: 106 g / mol)0.5 gr of a diprotic acid is dissolved in water and titrated with 10 mL 1 M KOH to phenolphthalein end point. What is the molar mass of the acid? ½ H2A (aq) + KOH (aq) --> ½ K2A (aq) + H2O (l) Molar mass of KOH: 56 gr/mol a. 100 gr/mol b. 50 gr/mol c. 200 gr/mol d. 150 gr/molFor an acid-base titration, the moles of the acid should be equal the moles of the base. 30 mL of aliquot of a 0.23N HCl is placed in an Erlenmeyer flask and 2 drops of phenolphthalein was added. It was titrated and had an intial reading of 15.8 The normality of the solution is found to be 0.52N. (a) How much of the NaOH solution is used for the titration? (b) What is the final reading on the buret?
- A 50.00 mL sample of a white dinner wine required 21.48 mL of 0.03776 M NaOH to achieve a faint pink color. Express the acidity of the wine in terms of grams of tartaric acid, H2C4H4O6 (M. M. = 150.10) per 100 mL of wine. Assume that the two acidic hydrogens are titrated at the end point. MM H2C4H4O6 = 150.10 MM NaOH = 40.00 Below is the balanced chemical equation for this titration.Consider the titration of the weak acid, benzoic acid, HC7H5O2. Its acid dissociation reaction is: HC7H5O2 (aq) + H2O (l) ↔ C7H5O2- (aq) + H3O+ (aq) A 25.00 mL sample of a solution of benzoic acid, concentration unknown, is titrated with 0.0500M NaOH solution. A plot of the titration is shown below. 1. what is the pKa (approximately) of benzoic acid? Its Ka? 2. on the plot, indicate the buffering region of the titration 3. From the pH at the equivalence point, estimate the pKb of benzoate ion (conjugate base to benzoic acid)______________[Remember, at the equivalence point, C7H5O2- (aq) + H2O (l) ↔ HC7H5O2 (aq) + OH- (aq) ]A substance contains 0.5 g of magnesium hydroxide as the only basic ingredient . The sunstamce is analysed by dissolving it and titrating with a standard hydrochloric acid solution .The hydrochloric acid solution used in this titration is made by diluting 200 ml of 2M standardised solution to 500 ml 1.Calculate the volume of the HCl solution required to neutralize two of these indigestion substaces dissolved in water to make 35ml solution and calculate the concentration of Cl- in the final solution in mol.dm-3
- 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?Normality is same as Molarity for sodium hydroxide and normal = molar (for NaOH) Normality of sodium hydroxide = 0.10395N (normal) or Molarity of NaOH = 0.10395M (molar) Volume of NaOH consumed during the titration = 21.87 mL Mol wt of Naproxen = 230.26 g/mol Weight of Naproxen ds (i.e., sample) = 0.534g Calculate the % Purity (dried-basis) of Naproxen ds, given that the LOD results for Naproxen = 1.0% a 97.0 b 98.0 c 98.5 d 99.0 e 99.5 f none of the other answers.A biochemist needs 750 mL of an acetic acid–sodiumacetate buffer with pH 4.50. Solid sodium acetate(CH3COONa) and glacial acetic acid (CH3COOH) areavailable. Glacial acetic acid is 99% CH3COOH by massand has a density of 1.05 g/mL. If the buffer is to be 0.15 Min CH3COOH, how many grams of CH3COONa and howmany milliliters of glacial acetic acid must be used?