Please rank from 1(lowest) to 4(highest). Thank you!! ACIDS AND BASESTeSearPredicting the qualitative acid-base properties of saltsConsider the following data on some weak acids and weak bases:acidbaseKanameformulanameformulaHCH;CO2|1.8× 10- 5-4acetic acidethylamine C2H,NH, 6.4x 10hydrofluoric acidHF-46.8 × 10NH3-51.8 × 10ammoniaUse this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next tothe solution that will have the next lowest pH, and so on.solutionpH0.1 M NH4CIchoose one0.1 М KNO3choose onev0.1 M NaFchoose one♥0.1 М КСН3СО2choose one♥?II

pH = -log[H+] HA = A- + H+ K is equilibrium constant K = [A-][H+]/[HA] pKa = -log Ka So,…

Consider the following data on some weak acids and weak bases: acid base K. K, name formula name formula НCH, CO1.8х 10 ethylamine C,H5NH, |6.4× 10 acetic acid hydrofluoric acid HF 6.8 × 10¯4 ammonia NH3 |1.8 × 10¬5 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 M NHẠCI choose one♥ 0.1 Μ KΝO3 choose one v 0.1 M NaF choose one v 0.1 M KCH3CO2 choose one v

Consider the following data on some weak acids and weak bases: acid base K. K, name formula name formula НCH, CO1.8х 10 ethylamine C,H5NH, |6.4× 10 acetic acid hydrofluoric acid HF 6.8 × 10¯4 ammonia NH3 |1.8 × 10¬5 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 M NHẠCI choose one♥ 0.1 Μ KΝO3 choose one v 0.1 M NaF choose one v 0.1 M KCH3CO2 choose one v

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 10RQ: For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen...

See similar textbooks

Similar questions

The following reactions illustrate Brnsted acid-base behavior. Complete each equation. a.HI(aq)+?H3O+(aq)+I(aq) b.NH3(l)+?NH4++NH2 c.H2C2O4(aq)+H2O(l)?+HC2O4(aq) d.H2N2O2(aq)+H2O(l)H3O+(aq)+? e.?+H2O(l)H3O+(aq)+CO32(aq)
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
The sec-butyl cation can react as both a Brnsted-Lowry acid (a proton donor) and a Lewis acid (an electron pair acceptor) in the presence of a watersulfuric acid mixture. In each case, however, the product is different. The two reactions are as follows: (a) In which reaction(s) does this cation react as a Lewis acid? In which reaction(s) does it react as a Brnsted-Lowry acid? (b) Write Lewis structures for reactants and products and show by the use of curved arrows how each reaction occurs.
1. Which of the following can act as a Lewis acid? (Hint : In each case, draw the Lewis electron dot structure of the molecule or ion. Are there lone pairs of electrons on the central atom? If so, it can be a Lewis base. Does the central atom lack an electron pair? If so, it can behave as a Lewis acid.) PH3 BCl3 H2S HS−
Oxalic acid (H2C2O4) is a diprotic acid with Ka1=5.6×10-1 and Ka2=1.5×10-4. Oxalate ion (C2O42-) also has two base dissociation constants, Kb(1) =6.5×10-11 and Kb2=1.8×10-14. Based on these values, deduce the formula to compute the base dissociation constants of oxalate ion in terms of Kw and Ka1 or Ka2.
The acid ionization constants for species that are listed below can be found by using data given in the following tables: Acid Ka1 Ka2 Ka3 H3PO4 7.5 x 10–3 6.2 x 10–8 4.2 x 10–13 H2CO3 4.3 x 10–7 5.6 x 10–11 HNO2 4.5 x 10–4 HIO3 1.7 x 10–1 Base Kb NH3 1.8 x 10–5 Which of the following is the weakest acid? HCO3– HNO2 NH4+ HIO3 H2PO4–
The value of Ka for acetic acid is 1.80×10-5.What is the value of Kb, for its conjugate base, CH3COO-?
Calculate the molar concentrations of C2H3O2-(aq) in a 0.350 molar acetic acid. The ionization constant of acetic acid is 1.8x10^-5
CH3COOH + H2O --> H3O+ + CH3COO- Meaured pH of solution= 2.58 10mL of 1M acetic acid a) Calculate the [H3O+] at equilibrium for this solution. (include units) b)Calculate the [CH3COO-] at equilibrium for this solution. (include units) c) What is the [CH3COOH] at equilibrium for this solution? (include units)
list the basicity States by explaining them from large to small.(base)
The Ka of the weak acid HSO4- (aq) is 1.2*10-2 Give the weak acid's conjugate base and calculate the congugate base's Kb.