You can obtain the pH of a 0.100 M HCl solution by assuming that all of the H3O+ ion comes from the HCl, in which case the pH equals –log 0.100 = 1.000. But if you want the pH of a solution that is 5.00 x 10-8 M HCI, you also need to account for H3 O+ ion coming from water. Note that the auto-ionization of water is the only equilibrium you need to account for. What is the pH of 5.00 x 10 3 м HC1? pH =

For the diprotic weak acid H2A, Ka1-3.4x10-6 and Ka2=6.1×10-9. What is the pH of a 0.0500 M solution of H2A? What are the equilibrium concentrations of H2A and A2- in this solution? Express Ka1 in terms of x, and then show the simplified expression (when x is assumed to be negligible compared to to the initial concentration). Kal-A/B =C/D numerator A in complete expression: denominator B in complete expression: numerator C in simplified expression: denominator D in simplified expression: Also, give the numerical value of x using the appropriate approximation. What is the pH of the solution if you stopped here? X: pH:

A solution of HCN was prepared in 2.5 L of water.  The pH of this solution at 25°C was determined to be 4.87. The Ka for hydrocyanic acid is 6.17 × 10-10. How many moles of HCN were used to prepare the solution? Report your answer to the hundredths place

At 25°C the value of Kw is 1.0 x 1014. At 60°C the value of Kw is 1.0 x 1013. Is the reaction exothermic or endothermic? Explain briefly. Calculate [H3O] and pH in a neutral solution at 60°C. 2H,0 0 H,O* (12)+OH (2)

Will 0.10 M aqueous solutions of the following salts be acidic, basic or neutral?

Can you provide an example and explanation?

Calculate the concentrations of all species in a 1.33 M NACH, COO (sodium acetate) solution. The ionization constant for acetic acid is K, = 1.8 x 10-5. [Na*] = M [CH,COO-] = M [OH¯] = M [CH, COOH] = M %3D [H,O*] = M

Calculate the pH of a solution that is 0.155 M in acetic acid and 0.255 M in sodium acetate. The Ka of acetic acid is 1.8 x 10^-5.

What is the pH of a solution that is 0.10 M potassium nitrite, KNO2 and 0.17 M HNO2? The Ka for HNO2 is 4.5x10-4. You do not need to solve the quadratic equation for this problem. Express your answer to two decimal places.

Calculate the concentrations of all species in a 0.300 M NaCH,COO (sodium acetate) solution. The ionization constant for acetic acid is K, = 1.8 × 10-5. [OH¯] = M [CH,COOH] = M [H,O*] = M