Answered: What is the Molar Mass (g/mol) of an…

What is the Molar Mass (g/mol) of an unknown monoprotic weak acid if 648 mg of it requires 35.86 mL of 0.1221 M NaOH to titrate it to equivalence (aq., 25 oC)?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.103QE: A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A...

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A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
ssume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 7.00 ✕ 102 mL of solution and then titrate the solution with 0.153 M NaOH. C6H5CO2H(aq) + OH-(aq) C6H5CO2-(aq) + H2O(ℓ) What are the concentrations of the following ions at the equivalence point? Na+, H3O+, OH-C6H5CO2- M Na+ M H3O+ M OH- M C6H5CO2-
Calculate the value of the equilibrium constant for the balanced net ionic equation for the weak acid- strong base titration. The beaker contains 0.1894 M CH3COOH and the buret contains 0.2006 M NaOH. 24 ml of NaOH is needed to titrate. lonic Equation: CH3COOH (aq.) + OH (aq.) = CH3 COO"(aq.) + H2O (1) Please help thank you.
4.48 The weak base colloquially known as Tris, and more precisely as tris(hydroxymethyl)aminomethane, has pKa = 8.3 at 20°C and is commonly used to produce a buffer for biochemical applications. (a) At what pH would you expect Tris to act as a buffer in a solution that has equal molar concentrations of Tris and its conjugate acid? (b) What is the pH after the addition of 3.3 mmol NaOH to 100 cm3 of a buffer solution with equal molar concentrations of Tris and its conjugate acid form? (c) What is the pH after the addition of 6.0 mmol HNO3 to 100 cm3 of a buffer solution with equal molar concentrations of Tris and its conjugate acid?
A 5.296 g sample of a solid, weak, monoprotic acid is used to make a 100.0 mL solution. 30.00 mL of the resulting acid solution is then titrated with 0.09755 M NaOH. The pH after the addition of 21.00 mL of the base is 5.02, and the endpoint is reached after the addition of 46.38 mL of the base. (a) How many moles of acid were present in the 30.00 mL sample? 0.004524 mol(b) What is the molar mass of the acid?351.1 g/mol(c) What is the pKa of the acid? just need help with part C
2) Titration of the diluted solution with hydrochloric acid 18ml of the diluted solution (S,) are transferred into a 250 ml beaker, then titrated with a solution of HCl of concentration C, = 0.018 mole/L. Using a pH-meter we follow the change of the pH of the mixture as a function of V. (the volume of acid added). The following results are tabulated: V, in ml 2 5 7 8 8.5 8.7 8.9 9. 9.1 9.3 9.5 10 11 13 15 pH 12 11.8 11.6 11.3 11 10.5 10.2 | 9.2 7 4 3.7 3.2 2.7 2.4 | 2.3 2.1- Indicate a convenient glassware that must be used to : 2.1.1 - Withdraw the volume of solution S, . 2.1.2- Add HCI solution 2.2-Write the equation of the titration reaction, list its characteristics. 2.3- Plot the curve pH = f(Va) abscissa 1 cm 1 ml and ordinate 1cm 1 pH units 2.4- Determine graphically the coordinates of equivalence point 2.5- Based on the chemical species present in the beaker, justify the value of the pH at equivalence point. 2.6- Determine the molar concentration of solution (S,). 2.7- Deduce…
A 5.145 g sample of a solid, weak, monoprotic acid is used to make a 100.0 mL solution. 27.00 mL of the resulting acid solution is then titrated with 0.09636 M NaOH. The pH after the addition of 16.00 mL of the base is 5.75, and the endpoint is reached after the addition of 45.85 mL of the base. (a) How many moles of acid were present in the 27.00 mL sample?4.42e-3 mol(b) What is the molar mass of the acid?314 g/mol(c) What is the pKa of the acid? (only confused on part c, answers for a and b are given)
a.) A student titrated 50.0mL of a 0.10M solution of a certain weak acid with NaOH(aq). The results are given in the graph attached. (i) What is the approximate pKa of the acid? (ii) What specific value from the graph is needed, in addition to the information in part (a) above, to calculate the molar concentration of the NaOH(aq) ? (iii) Identify a pH value between 2.5 and 7.5 at which the concentration of the weak acid being titrated is less than the concentration of its conjugate base.
Propionic acid, HC3H5O2, has a Ką value of 1.3 x 105. A buffer solution is prepared by mixing 20.0 mL of 0.100 M HC3H5O2(aq) with 10.0 mL of 0.100 M NaC3H502(aq), its conjugate base. The pH of this buffer solution is measured to be 4.59. What is the concentration (in M) of the acidic component of this buffer solution. Express your answer to 3 significant figures, using the
What volume of 0, 955 M HCI (in mL0 is required to titrate 2,152 g of Na2CO3 to the equivalence point? Na2CO3 (aq) + 2HCI (aq) - H2O (l) +CO2 (g) + NaCI (aq)
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).
Consider the titration of 36.0 mL of 0.123 M ammonia with 0.0766 M HCl. (See the Acid-Base Table attached.) (a) How many mL of HCl are required to reach the equivalence point?57.8 mL(b) What is the pH at the equivalence point? 5.29(c) What is the pH of the solution after the addition of 17.2 mL of acid? (d) What is the pH of the solution after the addition of 84.3 mL of acid? (only need help witn c and d)