In finding the pH of the solution containing amphiprotic salts, diluted solutions contain significantly lower molar concentration of the salts, resulting to negligible significance of Kw in the equation, thus [H3O'] is approximately equal to the square root of the first two acid dissociation constants. With this, calculate the hydronium ion concentration of a 0.100 M NaHCO3 solution, given that Kay = 1.5 x 104 and Kaz = 4.69 x 10¹" a. 8.4 x 10-8 M b. C. d. 8.1 x 10-¹0 M 8.5 x 10⁹ M 8.3 x 10-1¹ M

For each of the following entities • Identify it as a strong or weak acid. • Select the correct arrow to show the changes that occur when the acids are placed in water. • Select the approximate pH for each resulting solution. HCI(aq) is classified as a + acid. The reaction equation with water utilizes which of the following arrows? Choice A Choice B 7 >>7 H2SO3(aq) is classified as a The reaction equation with water would utilize which of the following arrows? Choice A Choice B < 50% H2SO3(aq) + H20(I) • HSO3 (aq) + H30*(aq) The approximate pH of the solution would be

Please don't provide handwritten solution

Calculate the degree of dissociation (%) for a 0.10 M aqueous solution of hydrogen cyanide (HCN) at a temperature, where its acid constant value is pKHCN = 9.2.

Calculate the pH of the amphiprotic salt NaHA.  Ka (H2A) = 0.0026, Ka (HA-) = 0.0000000077

Ammonium nitrate NH4NO3 is a salt used in fertilizers and in making matches. The salt is made by the reaction of ammonia, NH3 and nitric acid, HNO3. Calculate the pH of a 0.15 M solution of ammonium nitrate at 25o   Ka=5.6×10-10   NH4+ (aq) +H2O(l) → NH3 (aq) +H3O+ (aq)     pH=-log[H3O+]

Calculate the pH of a solution that is 1.8*10^-3 M morphine if the pKa of its conjugate acid is 8.21

On a shelf in the lab storeroom marked “Solutions of Acids”, a bottle has a torn label. All that can be seen on the label is the concentration:  643 x 10-3 M, not the name of the acid.  In trying to find the identity of the acid, you measure the pH of this solution and find it to be 3.382. Of the acids listed on the chart of Acid Dissociation Constants (attached), WHICH ACID could this be?  There is only one correct answer. Hint:  Use the given information to find Ka.  Use all sig figs in the pH.

pHpH is a logarithmic scale used to indicate the hydrogen ion concentration, [H+], of a solution: pH=−log[H+] Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, [OH−], are related to each other by the Kw of water: Kw=[H+][OH−]=1.00×10^−14 where 1.00×10^−14 is the value at approximately 297 K. Based on this relation, the pH and pOH are also related to each other as 14.00=pH+pOH The temperature for each solution is carried out at approximately 297 K where Kw=1.00×10^−14 A. 0.20 g of hydrogen chloride (HCl) is dissolved in water to make 5.5 L of solution. What is the pH of the resulting hydrochloric acid solution? B. 0.20 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution? C. Calculate the concentration of HSO4− ions in a 0.010 M aqueous solution of sulfuric acid.

We did an experiment in a lab. We tested for the strength of acids and bases using a conductivity test. Distilled water was used as one of the solutions. the litmus paper and phenolphthalein did not change color. It did not also conduct electricity. Hence it was assumed to be a nonelectrolyte therefore a neutral solution. However, upon searching the internet, it was found that water is not exactly acidic. A pH of 7 at 25°C represents PURE distilled water. Distilled water is considered to be slightly acidic because it absorbed carbon dioxide from the air. The pH of distilled water can range anywhere between 5.5 and 6.9, depending on how long it has been exposed to air. If this is true, then shouldn't the distilled water conduct electricity since acids conduct electricity? Yes or No? please provide an explanation and chemical equation if possible. thank you!