Balance the equation. Determine either the molarity or volume necessary to completely neutralize the acid or...
Balance the equation. Determine either the molarity or volume necessary to completely neutralize the acid or base. Compute the pH of the neutralized solution. K. (HX) = [H3O+][X-1/[HX] K, * K = K = 10-14 3. Ba(OH)2 + KHSO4 + Ba(KSO4)2 + H2O Ka(HSO4) = 1.0x102 Vo = 75.0 mL Mo = 4.0 V. = M = 0.667 M ?
Balance the equation. Determine either the molarity or volume necessary to completely neutralize the acid or base. Compute the pH of the neutralized solution. K, (HX) = [H3O+][X-1/[HX] K," K = K = 1044 1. KOH + HCOH – KOẠCH+ H2O Ka for formic acid = 1.8 x 10-4 Vb= 50.0 mL Mo = 2.2 M V = 80.0 mL M = ?
Balance the equation. Determine either the molarity or volume necessary to completely neutralize the acid or base. Compute the pH of the neutralized solution. K. (HX) = [H3O+][X-1/[HX) K, * Ko = K = 10-14 4. HCl + CsHsN (pyridine) → CsH3NH + Cl" K(pyridine) = 1.7x10-9 (C5H5N - C5H5NH + OH) Vo= mL M = 0.5 V. = 100. mL M = 0.667 M?
thank you <3
really struggling with the worksheet
Practice Problems What is the molarity of a solution of NaOH if 25 mL of 1.2 M HCI is required to neutralize 15 mL of the base? What valume of 1.5 M HCI is required to completely neutralize 1B ml, of 2.0 M KOH? Per f 25.)- How many mL of 3.0 M HNO, can be completely neutralized by 75 mL of 1.5 M Mg(OH)2 solution? If 150 mL of 1.0 M...
Part A. Calculate the volume lf 0.210-M NaOH solution needed to completely neutralize 89.1 mL of a 0.310-M solution of the diprotic acid H2C2O4 Part B. You wish to make a 0.202 M Hydrochloric acid solution from a stock solution of 3.00 M hydrochloric acid. How much concdntrated acid must you add to obtain a total volume of 50.0 mL of the dilute solution? Part C. an aqueous solution of barium hydroxide is standarized by titration with a 0.143 M...
What volume (in mL) of 0.100 M barium hydroxide, Ba(OH)b, is needed to completely neutralize 25.0 mL of 1. 0.100 M hydrochloric acid, HCI? (A) 12.5 mL (C) 50.0 ml What are the Bronsted-Lowry bases in this reaction? (B) 250 mL (D) 75.0 mL 2. NH,(aq) + H2O(l) 근 NH'(aq) + OH-(hq) (B) HO and NH4 D) NH. and OH (A) NH and OH (C) NH, and H.O 3. What is the conenration of hydroxide ion in 0.015 M HCI(aq)...
Stomach acid (HCI) is neutralized by a variety of commercial antacids. Determine how many grams of the active antacid ingredient Al(OH)3 would be necessary to neutralize the HCI in 50.0 mL of 0.01 00 M HCI (an approximation of the concentration of HCI in the stomach). 16. 3 HCI (aq) + Al(OH)3 (s) AICla (aq) + 3 H2O (I)
Stomach acid (HCI) is neutralized by a variety of commercial antacids. Determine how many grams of the active antacid ingredient Al(OH)3...
What is the net ionic equation for the neutralization reaction between a HI with NH3? HI (aq) + NH3 (aq) ⇌ NH4I (aq), HI (aq) + OH- (aq) ⇌ H2O (l) + I- (aq), H3O+ (aq) + OH- (aq) ⇌ 2 H2O (l) H3O+ (aq) = NH3 (aq) = NH4+ (aq) + H2O (l) Which statement about buffers is NOT true? A buffer can be made by neutralizing some of the weak base in solution by adding a strong acid,...
10. For an aqueous solution labeled "0.10 M potassium bromide," A) the pH is greater than 7. B) the pH = 13. D) the pH is less than 7. E) the pH = 7. C) the pH = 1. 11. For a 0.10 M solution of a weak acid, HA, with pKa = 6, which of the following is true? A) [HA] =[A-] B) [HA] does not equal [H3O+] C) [HA] =[H3O] D) [HA] = K E) [HA] = 0...
Weak Acid-Strong Base Titration Date Nanse PRE-LAB OUESTIONS 1 Calculate the molarity of a NaOH solution that was used to titrate 1.2 g of potassium acid phthalate if 37.50 ml of the base were reauired to get to the end point of the titration. 2 It takes 12.45 ml. of a 0.500 M NaOH solution larity of the acid to titrate 30.0 mL of acetic acid. What is the mo- 3. Using the titration curve below, calculate the K, of...