1. At equal concentrations, the amount of ionization of an acid depends on the Ka values of the acids, i.e. the ionization constant of the acid. Since, HBr completely dissociates and has a Ka value >1, thus, in the aqueous medium, it exhibits the highest degree of ionization in water.
2. Weaker the acid, higher the pH. In the given list of acids, all the acids apart from HF, have Ka values > 1, thus, are strong acids, where as Ka for HF = 6.6 x 10-4. Thus, its pH value would be the highest.
3. More the number of particles in a solution, lower is the freezing point. In the given list of acids, HClO4 and HCl are strong acids and HClO being the weakest. Thus, for same concentrations, HClO would not dissociate completely into ions and increase the freezing point.
14. Given equal concentrations of the following acids, which exhibits the greatest amount of ionization in...
i need help
you mix equal concentrations of the following reactants and products, will the reaction proceed to the left or to the right? Explain your answer briefly. (6 pts) (a) HF (aq) + NO3(a) HNO, (aq) + F (b) NH. (aq) + CO2(aq) HCO3' (aq) + NH3(aq) 17. The concentration of OH in human blood is 2.24 x 10-7M. Calculate the concentration of H30 ions and classify the solution as acidic, neutral or basic (5 pts) 18. (a) What...
please answer both questions
QUESTION 28 Which of the following acids HCIO2(aq) HClO(aq) HBrO2(aq) HBrO(aq) HIO(aq) is the strongest in aqueous solution? a HIO(aq) HCIO(aq) HBrO2(aq) HCIO2(aq) e. HBrO(aq) QUESTION 29 What is the pH of an aqueous solution of 0.184 M carbonic acid, H2CO3? (Kal - 4.2 х 10-7, ка2 - 4.8 x 10-11) Оа. 3.50 ОБ. 2.80 ОС- 3.56 Od. 2.69 Оe. 297
1) For the following reaction, which of the following is a conjugate acid-base pair? HC20(aq)+ H20) H:0 (aq) C0,(aq) a. HC20 and H20 b. H20 and C202 c. HC20 and H30 d. HCzOr and C20 2) The pH of a solution of hydrochloric acid is 1.5. What is the concentration of the acid? a. 0.22 mol/dm b. 0.32 mol/dm3 c. 3.2x 102 mol/dm d. 2.2x 10-3 mol/dm 3) Which of the following diagrams represents the acid with the highest pH?...
question 2 and 3 could be answer is a complete question
Part 2. (3pt) If we pump HF gas into the buffer solution in Part 1 (without changing the solution volume), which of the following statement should be true? Statement (I): The concentration of fluoride ion F will decrease. Statement (Il): The pH of the buffer will decrease. Statement (IIl): The concentration of H30* will decrease. a) (0) b) (l) c) (IlI) d)(0) and () e) (0) and (II) f...
6.16 Classify each of the following solutes as an electrolyte or a nonelectrolyte a. NaNO3 b. C6H12O6 c. FeCl3 6.26a Calculate the composition of 20.0 g acetic acid dissolved in 2.50 L in mass/volume% 6.28b Calculate the %m/m composition of 50.0 g KCl in 5.00 x 102 mL solution (d=1.14g/mL) 6.30a How many g of solute are needed to prepare 2.50x102 g of 5.00% (m/m) NH4Cl? 6.34 How many mL of 4.0 mass/volume % Mg(NO3)2 solution would contain 1.2 g...
I didn't know which one so I
posted all of what I was provided
Acid/Base Ionization Constants at 25 °C Acid Formula Kal Ka2 Каз Acetic acid CH3COOH 1.8x10-5 Acetylsalicylic acid (aspirin) HC,H-04 3.0x10-4 Aluminum ion Al(H20)43+ 1.2x10-5 Arsenic acid H3 AsO4 2.5x10-4 5.6x10-8 3.0x10-13 Ascorbic acid H2C6H606 7.9x10-5 1.6x10-12 Benzoic acid CH3COOH 6.3x10-5 Carbonic acid H2CO3 4.2x10-7 4.8x10-11 Ferric ion Fe(H20)63+ 4.0*10-3 Formic acid HCOOH 1.8x104 Hydrocyanic acid HCN 4.0*10-10 Hydrofluoric acid HF 7.2x104 Hydrogen peroxide H202 2.4x10-12 Hydrosulfuric...
Explain why some electrolyte solutions are strongly conducting, whereas others are weakly conducting. 4.2. Def fine the terms strong electrolyte and weak electrolyte. Give an example of each 4.3. Ex plain the terms soluble and insoluble. Use the solubility rules to write the formula of an insoluble ionic compound. 4.4. What are the advantages and disadvantages of using a molecular equation to represent an i reaction? 4.5. What is a spectator ion? IlIlustrate with a complete ionic reaction 4.6. What...
4.30. Using solubility rules, predict the solubility in water of the following ionic compounds. a. AI(OH) b. CaN C. NH4CI d. KOH 4.32. Using solubility rules, decide whether the following ionic solids are soluble or insoluble in water. If they are soluble, write the chemical equation for dissolving in water and indicate what ions you would expect to be present in solution. (NE SO b. BaCO c. Pb(NOs)2 d. Ca(OH) 4.34. Write net ionic equations for the following molecular equations....