Blood pH can be impacted by the carbonic acid/bicarbonate system, which utilizes the following formula:CO2 + H2O << H2CO3 « HCO3 + H*What effect would the IV bicarbonate have on the carbonic acid/bicarbonate reaction above?Shift it to the leftB Shift it to the right(C)Settle it closer to equilibriumNo effect.

Background: The carbonic acid/bicarbonate system is a major buffer system in the blood, helping to…

Answered: Blood pH can be impacted by the…

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter10: Potentiometry And Redox Titrations

Section: Chapter Questions

Problem 5P

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What are the products of each of the following acid-base reactions? Indicate the acid and its conjugate base and the base and its conjugate acid. (a) HCIO4 + H2O (b) NH4 ++ H2O (c) HCO3 + OH
4, . Consider the following equilibrium: base + -H H-Base Which of the following base(s) would favour the product in this reaction? Он CH;O NH3 NH2 CH3CO2 (1) (II) (III) (IV) (V) (a) | (b) IV (c) I, IV and V (d) I and II (e) IIl and IV
Write the basic equilibrium equation for C,H,NH, 3. O4- D2. O+ n2+ O3+ O4+ 1 2 3 4 7 8 1 3 4 5 O6 (s) (1) (g) (aq) + -> H C OH Reset • a H,O Delete 80 888 F3 F4 F5 F6 F7 FB 2# $ % & * 3 4 5 6 7 9 W E R Y U CO
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How do you solve for the constant equilibrium constant generally?
Write the basic equilibrium equation for C,0,. 04- 3. 2. O+ D2+ O3+ 04+ 1 2 4 6. 7 8 9. 04 Os O6 O8 (g) (aq) + (s) (1) H C OH H,O* Reset • x H¸O Delete 80 DII DD F3 F5 F6 F7 F8 # $ & 3 4 5 6 8 9 W E R T Y U 1
Fill in the correct “changes” in concentration terms for the following unbalanced equations, (e.g. “+y”, “-2y”, shown in bold in the Ex.) etc, in order to establish equilibrium.NOTE: if you start with a species on the product’s side, that side must lose an amount. Const. T & P. Example: 2 SO3ó 2 SO2 + Cl2(IS balanced) “x” “x” Change: +2y -2y -y a)CH4(g) + O2(g) ó CO2(g) + H2O(g)(unbalanced) “x”“x” Change:_______________ ______ b)H2O(g) + ó H2(g) + O2(g)(unbalanced) “x” “x” Change:__________ ______
Final Volume V₂ = 341 mL al Volume V₁ =? 10. What is the molecular geometry and molecular polarity for CH₂Cl, and SO, ²? 11. What do catalysts do and how do they affect reaction rates? 12. 2 Atoms are side by side. Their chemical reactivity is dependent on the electrons which hold serve fe 13. Identify the acid, base, conj. Acid, conj. Base: H₂CO, + HPO4 H₂PO4 + HCO, 14. True or False? Chemistry looks at the microscopic view of matter. 15. Identify the 4 biological buffer mechanisms 16. Calculate the density of silver metal if 930 cm³ block has a mass of 2.21 x 104 g. Express the answer with the correct number of significant figures. 17. Kinetic molecular theory describes the behavior of which state of matter? 18. The pH scale operates on a logarithm scale which means an increase or decrease fold in the of pH is by 10s. So, a change in pH from 5 to 3 is a hydrogen ion concentration. And in other words, a pH of 3 has and less OH- than a pH of 5 19. A precipitate occurs in the reaction…
The pka of ethanoic acid, (CH3COOH) (0.1 M), is 2.6 at 25°C. Write the balanced chemical equation for the ionisation of CH3COOH. a. b. C. Ka = Write the expression for the equilibrium constant, Ka Complete the initial-change-equilibrium table for the species in the reaction Conc (mol L-1) CH³COOH CH³COO¯ H³O+ Initial 0.100 Change Equilibrium CH3COOH + H3O+ 0.1-x +X CH3COO- 0 OH- [CH3COOH] [CH3COO-] + 0.2 -0.1 -X H3O+ H₂O H₂O
1
Be sure to answer all parts. Consider the formation of ammonia in two experiments. (a) To a 1.00-L container at 727°C, 1.30 mol of N₂ and 1.65 mol of H₂ are added. At equilibrium, 0.100 mol of NH3 is present. Calculate the equilibrium concentrations of N₂ and H₂ and find Ke for the reaction: [N₂ leq = [H₂ leq 2 NH3(g) = N₂(g) + 3 H₂(g) Kc = ㅈ = M Kc = (b) In a different 1.00-L container at the same temperature, equilibrium is established with -2 8.34 × 10² mol of NH3, 1.50 mol of N2, and 1.25 mol of H₂ present. Calculate Ke for the reaction: M 3 NH3(g) = N₂(g) + H₂(g) 2 2 C C < Prev *********** 18 of 20 MacBook Pro Search or type URL Next *********** ☆
1. H;Og) 2 H;SO41) + At equilibrium [S0;] = 0.400M [H;O] = 0.480M [H;SO4] = 0.600M Calculate the value of the equilibrium constant.

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