🌙 Calculate Ph Of Hno3

Transcribed image text: What is the pH of a 0.020 M HNO3 solution? O A. 12.30 O B. 1.70 O C. 0.020 O D. 0.040 What is the strongest acid among the following? O A. HI O B. HE O C. HBO O D. HCI. First thing first, calculate the total volume of the resulting solution. #V_"total" = "100.0 mL + 50.0 mL + 100.0 mL"# #V_"total" = "250.0 mL"# Now, you are dealing with two strong acids that ionize completely in aqueous solution. Both nitric acid and hydrochloric acid produce hydronium cations in #1:1# mole ratios, so you know that As mass / volume = molarity × molar mass, then mass / (volume × molar mass) = molarity. Substitute the known values to calculate the molarity: molarity = 5 / (1.2 × 36.46) = 0.114 mol/l = 0.114 M. You can also use this molarity calculator to find the mass concentration or molar mass. Simply type in the remaining values and watch it do all Explain. A 0.1M solution of an acid with Ka = 1 \times 10 - 4 K a= 1×10−4 or one with Ka = 4 \times 10 - 5 K a = 4×10−5. 1 / 4. Find step-by-step Chemistry solutions and your answer to the following textbook question: Calculate the pH of each aqueous solution: (a) 0.015 M HNO3; (b) 0.0025 M NaOH.. This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Question: Part B Calculate pH of the solution on addition of the following. 0.001 mol of HNO3 Express your answer using three significant figures. Calculate the pH for the strong acid/strong base titration between 50.0 mL of 0.100 M HNO 3 (aq) and 0.200 M NaOH (titrant) at the listed volumes of added base: 0.00 mL, 15.0 mL, 25.0 mL, and 40.0 mL. Answer to Solved Calculate th pH of 0.00756 M HNO3.. based on rules. This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. 1)Calculate the pH of a 0.1M solution of NaOH ,knowing that the volume of the solution is 300mL. 2)Calculate the pH of a 0.3M solution of HCl , knowing that the volume of the solution is 250mL (?) A solution contains #[OH^-] = 4.0 times 10^-5# #M#, what is the concentration of #[H_3O^+]#? Explanation: We use the pH equation, which states that. pH = −log[H +] or pH = − log[H 3O+] It is the same equation anyways, as water can dissociate two ways. Since the hydrochloric acid has a concentration of 0.34 M, that must mean that the concentration of hydronium (H 3O+) ions is also 0.34 M, i.e. there exists 0.34 moles of hydronium Ukhnv.

calculate ph of hno3