Complete the balanced chemical equation for the following reaction between a weak base and a strong acid. KNO,(aq) + H¸SO,(aq) –

Acetylsalicylic acid (C₂H8O4) is a monoprotic acid commonly known as aspirin. A typical aspirin tablet, however, contains only a small amount of the acid. In an experiment to determine its composition, an aspirin tablet was crushed and dissolved in water. It took 5.10 mL of 0.1466 M NaOH to neutralize the solution. Calculate the number of grains of aspirin in the tablet. (One grain = 0.0648 g and the molar mass of aspirin = 180.15.) mol Round your answer to 3 significant digits. grains ☐ ☐x10

By titration, it is found that 35.3 mL of 0.141 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCI solution. [HCI] = = 0.1 Incorrect M

Write the molecular equation, the total ionic equation (TIE) and the net ionic equation (NIE) for the reaction of aqueous solutions: phosphoric acid and sodium hydroxide.

(b) To neutralize 25.0 mL of a solution of the triprotic acid H3PO4(aq), we require 18.8 mL of a 0.555 M solution of Ba(OH)2(aq). What was the original concentration of H3PO4(aq)?

|A 500-g sample of Al, (SO, ); is reacted with 450 g of Ca(OH),. A total of 596 g of CaSO, is produced. Al, (SO4)3(ag) + 3Ca(OH) 2(aq) →2AI(OH) 3(s) + 3CaSO (s) Determine the following:

Using your knowledge of and bases, write balanced equations for the following acid-base reactions and indicate which reactant is the acid and which is the base. Write the molecular, ionic, and net ionic equations.    HNO3 (aq) + Ca(OH)2  (aq) → H2SO4 (aq) + KOH (aq) → CH3COOH (aq) + NaOH (aq) →

Balance the following equation, classify the reaction as combination, decomposition, single displacement, or double displacement, and write the total ionic equation and net ionic equation.

What would be the net ionic equation?

By titration, it is found that 66.5 mL of 0.158 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.