A buffer is prepared by combining 17.6 g of H2CO3 (carbonic acid) with 220 mL of 0.18 M NAOH and diluting to 3.5 L. (K, = 4.3 x 107) (MM H2CO3 = 62 g/moll) %3D a) Calculate the initial moles of acid (before reaction) (. b) Calculate the initial moles of the OH base (before reaction) c) Calculate the moles of H2CO3 and the conjugate base HCO3 after reaction( d) Calculate the concentrations H2CO3 and the conjugate base HC03 after the reaction e) Determine the pH of the buffer H,CO, + OH 2 HCO, + H,0 Initial moles a b After reaction Concentration

A buffer is prepared by combining 17.6 g of H2CO3 (carbonic acid) with 220 mL of 0.18 M NAOH and diluting to 3.5 L. (K, = 4.3 x 107) (MM H2CO3 = 62 g/moll) %3D a) Calculate the initial moles of acid (before reaction) (. b) Calculate the initial moles of the OH base (before reaction) c) Calculate the moles of H2CO3 and the conjugate base HCO3 after reaction( d) Calculate the concentrations H2CO3 and the conjugate base HC03 after the reaction e) Determine the pH of the buffer H,CO, + OH 2 HCO, + H,0 Initial moles a b After reaction Concentration

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 75QAP: A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this...

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Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

A buffer is prepared by combining 17.6 g of H2CO3 (carbonic acid) with 220 mL of
0.18 M NAOH and diluting to 3.5 L. (K, = 4.3 x 10 7) (MM H2CO3 = 62 g/moll)
%3D
a) Calculate the initial moles of acid (before reaction) (.
b) Calculate the initial moles of the OH base (before reaction)
c) Calculate the moles of H2CO3 and the conjugate base HCO3 after reaction
d) Calculate the concentrations H2CO3 and the conjugate base HCO, after the
reaction
e) Determine the pH of the buffer
H,CO,
Н,СО, + ОН 2 НСО, + Н,О
H,0
Initial moles
b
a
After reaction
Concentration
d.

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“Tris” is short for tris(hydroxymethyl)aminomethane.This weak base is widely used in biochemical research forthe preparation of buffers. It offers low toxicity and a pKb(5.92 at 25°C) that is convenient for the control of pHin clinical applications. A buffer is prepared by mixing0.050 mol of tris with 0.025 mol of HCl in a volume of2.00 L. Compute the pH of the solution.
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By mixing 3L of 2M H2SO4 and 4L of 2M NH4OH , the produced solution will be ......... a) Acidic b) Basic c) Neutral
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71tIN31Mrr15eZ41AWW-Ty2kfKY-gdiBaAX2wU/edit=slide%=Did gc31407e235 0_39 SS.. Typing Spanish Ac.. D Prese Is Add-ons Help Last edit was seconds ago 田 Background Layout- Theme Transition 1 2 3 I 4 5 6. 7 T 8 9. Drawing Conclusions How are 0.010 M solutions of HCI, CHOOH, and CH COOH similar to one another besides their concentration/molarity (M)? (Look at the ions present) 1. 2. How are they different besides what they are made up of? (Looks at the ions present)
the answer) Calculate the pH of a buffer that is 0.158 M HCIO and 0.099 M NaCIO. The K₂ for HCIO is 2.9 x 10-8. (3 sig figs in . Calculate the pH after 10 mL of 1M HCI is added to the buffer if it was a 1 L solution.
What quantity in moles of CHINH CI need to be added to 200.0 mL of a 0.500 M solution of CH3NH: (Kb for CHINH₂ is 4.4 x 10) to make a buffer with a pH of 11.05?
1. Which of the following salts, when dissolved in water, produce the basic solutions? (select all that apply, wrong choices will be penalized) NH4NO3, CsNO3, NaCl, K2CO3, NH4Cl, KI, NaC2H3O2, KCN, NH4ClO4 2. How many of the following pairs could be used to create a buffer if mixed in a 1:1 mole ratio? (select all that apply, wrong choices will be penalized) KOH and HNO3 HCl and NaCl H2CO3 and KHCO3 HCl and NaOH HF and NaF NH4Cl and NH3 HNO2 and NaNO2 HCl and NH3 HC2H3O3 and KC2H3O3
a) 1.00L of a buffer is created to be 0.100M in HOAC and 0.100M in NaOAc. What is the pH of the buffer? Ka = 1.8 x 10-5 b)Calculate the pH after adding 0.0200mol NaOH to the solution in (a) c)Calculate the pH after adding 0.0200mol HCI to the solution in (b) d) Is the buffer effective? Explain your answer (3-5 sentences) %3D
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