Calculate [OH⁻] in a solution obtained by adding 1.70 g solid KOH to 1.00 L of 10.0 M NH₃. (Kb of NH₃ is 1.80 × 10⁻⁵).

What is the concentration (in molarity) of H+, HCO3−, and CO32–, in a solution that is initially prepared as a mixture of 0.0100 M H2CO3 and 0.000010 M Na2CO3? (Carbonic acid is a weak diprotic acid where   Ka1 is 4.20 x 10–5 and Ka2 is 2.00 x 10–6)   a) [H+] at equilibrium = ? b) [HCO3-] at equilibrium = ? c) [CO32-] at equilibrium = ?

Complete the following neutralization reaction.  (Predict the products and balance the reaction.)    Ca(OH)2  +  HClO4   -->  ? Group of answer choices Ca(OH)2  +   HClO4   -->  2 H2O  +  CaClO4 Ca(OH)2  +   HClO4   -->   H2O2  +  CaClO4 Ca(OH)2  +   HClO4   -->   H2O  +  Ca(ClO4)2 Ca(OH)2  +  2 HClO4   -->  2 H2O  +  Ca(ClO4)2

The sample of 30.00 mL of 0.015 M HClO is titrated with a 20.00 mL of a 0.015 M NaOH solution. (a) Show the reaction between HClO and OH–.  (b) What is the final volume after two solutions were mixed?      (c) What is the final molarity of HClO after the reaction with OH–?     (d) What is the pH after 20.0 mL of the NaOH solution is added? (Ka of HClO is 3.0*10–8)?

A 1.631 g sample of an unknown triprotic acid (H3A) was dissolved in water and diluted to 250.0 mL in a volumetric flask. 20.00 mL of the acid solution required 19.74 mL of 0.1063 M NaOH to reach the endpoint of the titration. Determine the molar mass of the triprotic acid. Using a sketch might help!Write the balanced reaction

A 50.00-mL sample of a white dinner wine required 24.57 mL of 0.03291 M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated).

10g of the strong base Ba(OH)2 is dissolved in 200 mL of water and then titrated with 0.100 M HCl. How many mL of the acid solution must be added to exactly neutralize the solution?

The sample of 25.0 mL of 0.0200 M NH3 is titrated with a 20.0 mL of 0.0150 M HCl solution. (a) Show the reaction between NH3 and H+.  (b) What is the final volume after two solutions were mixed? (c) What is the final molarity of NH3 after the reaction with H+? (d) What is the pH after 20.0 mL of the HCl solution is added? (Ka of NH4+ is 5.6 x 10–10)

1. If 30.00 ml of a 0.300 mol/L of a weak acid, CH,CO,H (aq), is titrated with a 0.300 mol/L NaOH(aq), a strong base, determine the amount/moles and pH of the remaining acid after K, = 1.8 x 10* (a) 0.00 mL of NaOH is added (b) 10.00 mL of NaOH has been added. O at equivalency point when 30.00ml of NaOH was added. (d) Explain why the pH differs in (b) and (c)

Consider the following reactions: Reaction 1: HCIO, + KOH → KC1O, + H;O Reaction 2: HC;H;O2 + KOH → KC;H;O2+ H;O In both reactions, 15.00 mL of 0.8116 M acid is titrated with 0.4217 M KOH. A volume of 28.87 mL of KOH is required to reach the equivalence point in both reactions. a) What is the pH of the HC1O, solution before the titration has started? (No KOH has been added.) b) What is the initial pH of HC;H;O2 solution before the titration has started? K= 6.46 x 10-5 (Ok to use x is small.) c) What is the pH of Reaction 1 at the equivalence point? d) What is the pH of Reaction 2 at the equivalence point? e) What is the pH of Reaction 1 after 32.00 mL of KOH has been added? f) What is the pH of Reaction 2 after 18.00 mL of KOH has been added?