In each of the following acid-base reactions, identify the Brønsted acid and base on the left and their conjugate partners on the right.C; H;N(aq) + CH; CO,H(aq) 2 C;H;NH (aq) + CH3 CO, (aq)a.C; H;NCH3 CO,HC; H; NH+CH; CO2-b.H2PO, (aq) + N2H4 (aq) 2 HPO,² (aq) + N2Hs† (aq)H2PO4N2H4HPO,2N2H5+

According to Bronsted-Lowry theory, Acid is species which donates proton and Base is species which…

Answered: In each of the following acid-base…

Chemistry

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Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question 8 of 20 Sub Complete the balanced molecular reaction for the following weak base with a strong acid: NaCIO2(aq) + H2SO«(aq) – 3- 2. 2+ 3+ 4+ 04- 1 6 7 8. 9. 01 D 07 9. 2 3 4. 6. (s) (1) (g) (aq) -> Na H2O H3O* OHT H. CI • x H2O Delete Reset W ? Questions prep ok étv A 山 T。 OCT 4. MacBook Pro 8. 11
Write the formulas of the conjugate acids of the following Brønsted-Lowry bases: (a) CICH,CO, (c) SeO, (b) C;H;N 2- (d) (CH;),N
Benzoic acid, C,H,COOH, is a weak acid with K, = 6.3 × 10-5. CH,CO,H(aq) + H,O(1) H;O*(aq) + CH;CO,-(aq) 1. Calculate the pH of a 0.150 M benzoic acid solution. Show all calculations.
Which of the following equations represents the acid equilibrium associated with Ka, for H3PO3? A) HPO,²- (aq) + H20 (1) = PO;3- (aq) + H;0* (aq) B) H;PO, (aq) + H,0 (1) = H,PO;¯ (aq) + H,0* (aq) = H¿PO;- C) H,PO,- (aq) + H,0 (1) = H,PO3 (aд) + ОН- (аq) D) H,РO;- (аq) + H,0 () (aq) + H30* (aq) HPO,2-
Consider the following data on some weak acids and weak bases: acid base 9. name formula name formula HNO, 4.5 x 10 C;H;N |1.7× 10 nitrous acid pyridine hypochlorous acid 8. HСIО |3.0х 10 methylamine CH;NH, |4.4 × 10-4 Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 М KCIO v choose one 1 (lowest) 0.1 M C5H5NHCI 3 0.1 M NaNO2 4 (highest) 3 0.1 М KNO3 choose one
Complete the balanced molecular reaction for the following weak base with a strong acid: Na CIO2(aq) + H2SO«(aq) – 4- |2+ 3+ 04+ 1 4 6. 7 8 9 Do (s) (1) (g) (aq) Na CI S H H2O OH Reset x H2O Delete 1L LO
The pH of a 1.00 M NaCH3COO (aq) solution is 9.38. a/ Determine the concentration of [OH-] in the solution. b/ Write the expression for the Kb of NaCH3COO (aq) and calculate its values. c/ Calculate the pKa of CH3COOH. d/ HCl (aq) is added to 1.00 L solution of 1.00 M NaCH3COO (aq). Write the chemical reaction between HCl (aq) and NaCH3COO (aq). e/ How many mol of HCl (aq) is needed to make a buffer solution with pH = 5.00 from 1.00 L of 1.00 M NaCH3COO (aq).
4. The equations and constants for the dissociation of three different acids are given below. HCO3 = H+ + CO?- K. = 4.2 x 10–7 -8 H;PO, = H+ + HPO- K. = 6.2 x 10 HSO, = H+ + SO?- Ka = 1.3 x 10–2 a. From the systems above, identify the conjugate pari that is best for preparing a buffer with a pH. of7.2. Explain your choice. b. Explain briefly how you would prepare the buffer solution described in (a) with the conjugate pair you have chosen. c. If the concentrations of both the acid and the conjugate base you have chosen were doubled, how would the pH be affected? Explain how the capacity of the buffer is affected by this change in concentrations of acid and base.
15D.5.What is the difference between (a)monoprotic acid and a diprotic acid,(b) a weak acid and a strong acid, (c)an acid and a base? HCl, HBr, and HI are strong acids,yet HF is a weak acid. What does thismean in terms of the extent to whichthese substances are ionized insolution?Label each of the followingsubstances as an acid, base, salt, ornone of the above. Indicate whetherthe substance exists in aqueoussolution entirely in molecular form,entirely as ions, or as a mixture ofmolecules and ions. (a) HF; (b)acetonitrile, CH3CN; (c) NaClO4; (d)Ba(OH)2.
Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. C5H;NHI 2- + 2+ 3+ 4+ 1 2 3 4 6. 7 8 9 1 3 04 O6 O7 + (s) (1) (g) (aq) C OH H. NR H2O H30* N Reset • x H2O Delete LO 3.
The base protonation constant K, of allantoin (C,H,N,0,NH,) is 9.12 × 10 °. 4 3 3 Calculate the pH of a 1.3 M solution of allantoin at 25 °C. Round your answer to 1 decimal place.
In the reaction, HSO (aq) + OH(aq) = pair 1 pair 2 SO42- (aq) + H₂O(, the conjugate acid-base pairs are

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