Which solution is basic? A) pH = 3.00 B pH = 10.00 C) pH = 5.00 D) pH = 1.00 E p
ID: 511777 • Letter: W
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Which solution is basic? A) pH = 3.00 B pH = 10.00 C) pH = 5.00 D) pH = 1.00 E pH = 4.00 What is the pH of a 0.056 M HNO_3 solution? A) 0.056 B) 2.88 C) 12.75 D) 1.25 E) 11.11 Which is the net ionic equation for the reaction between aqueous solutions of lithium hydroxide and hydrobromic acid? LiOH(aq) + HBr(aq) rightarrow H_2O(l) + LiBr(aq) A) Li^+ (aq) + OH^- (aq) + H^+(aq) + Br^-(aq) rightarrow H_2O(l) + LiBr(aq) B) H^+(aq) + OH^-(aq) rightarrow H_2O(l) C) Li^+(aq) + Br^-(aq) rightarrow LiBr(aq) D) LiOH(aq) rightarrow Li^+(aq) + OH^-(aq) E) HBr(aq) rightarrow H^+(aq) + Br^-(aq) What is the [H^+] in a solution with a pH of 5.63? A) 2.344 times 10^-6 MH^+ B) 2.3 times 10^-6 MH^+ C) 2.3 times 10^-6 M H^+ D) 5.63 MH^+ E) 2.3 times 10^-5 M H^+ Automobile batteries use 3.0 M H_2SO_4 as an electrolyte. How much 1.20 M NaOH will be needed to neutralize 225 mL of battery acid? H_2SO_4 (aq) + 2NaOH (aq) rightarrow 2H_2O(l) + Na_2SO_4(aq) A) 0.56 L B) 1.1 LExplanation / Answer
22) B) PH = 10.00 The solutions which has a PH level above 7 is basic.
23) D)1.25 HNO3 exists as [H]++[NO3]- as it is a strong acid. To convert molarity to PH : PH = -log( .056) = 1.25
24) B)H+(aq) + (OH)-(aq) ---> H2O (l)
In a net ionic equation any ions which donot change are omitted .Li+ and Br- present initially convert to LiBr but as they are in solution they remain as Li+ and Br- itself and no net changes occur for these ions and the equation becomes H+(aq) + (OH)-(aq) ---> H2O (l)
25) A) 2.344 x 10-6 MH+ . Concentration of H+ = 10-(pH) = 10-(5.63) = 2.344 x 10-6
26) D) 0.28L
Using the equation N1V1 = N2V2 ,where N1 = the normality of H2SO4 which is 3/2 = 1.5( as acidity of H2SO4 is 2) , V1 = the volume of H2SO4 in liters = .225L , N2 = the normality of NaOH = 1.2 ( basicity of NaOH is 1) and V2 is the required volume.
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