Write the formula of the conjugate base of C6HSNH2.

Calculate the pH of a solution by dissolving 1.90 g of sodium acetate, CH3COONa, in 71.0 mL of 0.15 M acetic acid, CH3COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. Last of CH3COOH is 1.75 x 10^-5

Complete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. NH3(aq) + HCl(aq) – ->

The acid dissociation constant K of hydrocyanic acid (HCN) is 6.2 × 10¯¹⁰. Calculate the pH of a 6.9M solution of hydrocyanic acid. Round your answer to 1 decimal place.

Suppose a 0.25 M aqueous solution of phosphoric acid (H3PO4) is prepared. Calculate the equilibrium molarity of HPO4 2−. You'll find information on the properties of phosphoric acid in the ALEKS Data resource. Round your answer to 2 significant digits.

Complete the balanced chemical equation for the following reaction between a weak acid and a strong base  CH3NH3Cl(aq) + NaOH(aq) ->

The value pKw is 11.05 at 78 °C. What is the pH of a neutral solution at the same temperature? Enter your answer with two decimal places.

The chemical formulae of some acids are listed in the first column of the table below, and in the second column it says whether each acid is strong or weak. Complete the table. List the chemical formula of each species present at concentrations greater than about 106 mo mo-when about a tenth of a mole of the acid is L dissolved in a liter of water. The chemical formulae of some acids are listed in the first column of the table below, and in the second column it says whether each acid is strong or weak. Complete the table. List the chemical formula of each species present at concentrations greater than about 10-6 mol/L when about a tenth of a mole of the acid is dissolved in a liter of water. acid strong or weak? species present at 10-6 mol/L or greater when dissolved in water ICIO weak H₂SO, weak IICI strong HCIO, strong ☐ x DO....

What is the conjugate acid for H_2SO_3(aq)?

pH = −log[H+] where [H+] is the hydrogen ion concentration, measured in moles per liter. Solutions with a pH-value of less than 7 are acidic; solutions with a pH-value of greater than 7 are basic; solutions with a pH-value of 7 (such as pure water) are neutral. Black coffee has a pH of 5 and pure water has a pH of 7. Compare the pH of each and determine how much more acidic black coffee is than pure water.