Four solutions of an acid dissolved in water are sketched below, as if under a microscope so powerful individual atoms could be seen. The same volume of solution is shown in each sketch. Rank the solutions by the strength of the dissolved acid. That is, select 1 under the solution of the strongest acid, 2 under the solution of the next strongest acid, and so on. %3D Н,о Note: Solution 1 Solution 2 (Choose one) (Choose one) Solution 3 Solution 4 (Choose one) (Choose one)

8. The following pictures represent aqueous solutions of binary acids of the type HA where the Water molecules have been omitted for clarity. Which acid is the strongest acid of the set. = HA = H,0* = A %3D %3D A C D

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What salt is produced when each of the following acids and bases are mixed. Sodium HydroxideNaOHmixed with perchloric acidHClO4. Potassium hydroxideKOHmixed with hydrobromic acidHBr. Calcium hydroxideCa (OH)2mixed with hydrochloric acidHCl.

In an aqueous solution of a certain acid the acid is 0.083% dissociated and the pH is 4.20. Calculate the acid dissociation constant K of the acid. Round your answer to 2 significant digits. K= x10 $ ? X

What is the pH of an aqueous solution with [H3O+] = 2×10−14 M? Express the pH numerically using one decimal place.

Conjugate acid of any base is defined as the species formed when the base accepts a proton. And the conjugate base of any acid is defined as the species formed when the base donates a proton. Hence in the conjugate acid-base pair, there will be a difference of 1 proton only. In the above reaction, the base NH3 is accepting a proton from the acid HF to form + NH4* ions. Hence NH3/NH4* is a conjugate acid-base pair. And the acid HF is donating a proton to form the conjugate base F. Hence HF/F is a conjugate acid-base pair. Hence the answer is NH3/NH4* & HF/F". ANSWER IN NO. 4

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For a certain acid pK = decimal places. pH = 0 4.49. Calculate the pH at which an aqueous solution of this acid would be 2.9% dissociated. Round your answer to 2 X 5

Strong acids and strong bases ionize 100% in aqueous solution.- HCl is a strong acid. In solution we write it as H+(aq) + Cl -(aq).- HF is a weak acid. In solution we write it as HF(aq).- KOH is a strong base. In solution we write it as K+(aq) + OH -(aq).- NH3 is a weak base. In solution we write it as NH3(aq).Exception: Since Ca(OH)2 is only slightly soluble we write it as Ca(OH)2(s).Below is a list of the 6 strong acids and 6 strong bases you should know. All other acids and bases are considered weak. Strong Acids Strong Bases HCl, HBr, HI LiOH, NaOH, KOH HNO3 Ca(OH)2 (slightly soluble) HClO4 Ba(OH)2 H2SO4 Sr(OH)2 Question 1)What is the hydronium ion concentration in an aqueous hydrobromic acid solution that has a pOH of 10.200?[H3O+] =  M