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. Note: = H,0 Solution 1 Solution 2 hoose one) (Choose one) Solution 3 Solution 4 (Choose one) (Choose one)

Consider a solution which is [OH-] = 8.4 x 10-11 M. Calculate the [H3O+].

Assuming complete dissociation, what is the pH of a 4.12 mg/L Ba(OH)₂ solution? pH =

1a) The hydronium ion concentration of an aqueous solution of 0.394 M diethylamine (a weak base with the formula (C2H5)2NH) is[H3O+] = ______ M. b) The pOH of an aqueous solution of 0.394 M ethylamine (a weak base with the formula C2H5NH2) is ______

According to the Bronsted Lowry definition of an acid, in the reaction below, HC,H3O2 is considered an acid because-- HC2H3O2 → H* + C2H3O2 O It accepts a proton. O Increases the hydroxide ion concentration. O It donates a proton. O It increases the hydrogen ion concentration

Which of the following shows the correct relationship between the ions in aqueous solutions at 25°C? ) [H30*1×[OH¯] = 1.0 x 10-7 2) [H,o"] + [OH] = 1.0 x 10-14 3 [H30"]< [OH] = 1.0 x 10-14 4 [H,0"] ÷ [OH] = 1.0 x 10-14 5 [H30"] x [OH] = 1.0 x 10-14

What is an acid-base reaction? Match the items in the left column to the appropriate blanks in the sentences on the right. a precipitate a new acid or a new base OH- H₂O(1) H+ When an acid and base are mixed, the from the base to form from the acid combines with the Reset Help

Each row of the table below describes an aqueous solution at about 25 °C. Complete the table. That is, fill in any missing entries in the second and third columns. Round your entries for H,O' to 2 significant digits, and your entries for pH to 2 decimal places. solution pH K10 A 6.2 x 10 mol/L |mol/L 8.48 7.8 x 10 mol/L

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НА А- - H+ HB НА H* A- HB HB H* B- B- Figure 1 Figure 2 Which process shows the dissociation for a weak solution? Explain.