🦘 Calculate Ph Of Hno3

Question 1 Calculate the pH of a 1.0 × 10−6M solution of HNO3 Question 2 Calculate the pH of a 1.0 × 10−1M solution of NaOH This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Calculate the pH of 0.100 L of a buffer solution that is 0.20 M in HF (Ka = 3.5 x 10-4 ) and 0.47 M in NaF. Express your answer using three significant figures. pH = 3.83 Part B What is the pH after adding 0.003 mol of HNO3 to the buffer described in Part A? Express your answer using three significant figures. Calculate the pH value of 0.001 N `HNO_(3)` solution. asked Feb 12, 2022 in Chemistry by Harshitagupta (25.0k points) class-11; equilibrium; 0 votes. 1 answer. Caculate the pH of 0.001 N `H_(2)SO_(4)` solution. asked Dec 10, 2019 in Chemistry by AasaSinha (73.5k points) class-11; equilibrium; 0 votes. 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 HNO 3 + H 2 O -> H + + NO 3-. This means that for every 1 mole of HNO 3 that dissociates, 1 mole of H + is produced. Thus, every 0.0040M of HNO3 produces 0.0040M of H+. Perfect! Now we can plug our [H+] into the formula for pH: pH = -log [H+] pH = -log [0.0040M] pH = 2.397940009. We have 2 significant figures (sig figs) in our given value 0 Consider the titration of 100.0 mL of 0.100 M H»NNH, (K) = 3.0 x 10-6) by 0.200 M HNO3. Calculate the pH of the resulting solution after the following volumes of HNO3 have been added. a. 0.0 mL pH b. 20.0 mL pH = c. 25.0 mL pH = d. 40.0 mL pH = e 50.0 ml solution after the following volumes of HNO3 have been added. ? a. 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 Some chemists and analysts prefer to work in acid concentration units of Molarity (moles/liter). To calculate the molarity of a 70 wt. % nitric acid the number of moles of HNO 3 present in 1 liter of acid needs to be calculated. Knowing the density of the acid to be 1.413 g/mL, we can calculate the weight of 1 L of 70% HNO 3 to be 1413 Chemistry. Chemistry questions and answers. Calculate the pH of the solution after the addition of each of the given amounts of 0.0682 M HNO3 to a 70.0 mL solution of 0.0750 M aziridine. The p𝐾a of aziridinium is 8.04. What is the pH of the solution after the addition of 0.00 mL HNO3? Chemistry questions and answers. 5. Calculate the pH of a 0.025 M solution of HNO3. HNO3 is a strong acid. (5 Points 6. Calculate the pOH and pH of a 0.004 M solution of KOH. KOH is a strong base. (5 Points) "pH" = 1.222 As you know, sodium hydroxide and hydrochloric acid neutralize each other in a 1:1 mole ratio as described by the balanced chemical equation "NaOH"_ ((aq)) + "HCl"_ ((aq)) -> "NaCl"_ ((aq)) + "H"_ 2"O"_ ((l)) This means that a complete neutralization, which would result in a neutral solution, i.e. a solution that has "pH" = 7 at room temperature, requires equal numbers of moles of 12/12/2023, 8:18:01 AM. To prepare 1000 mL of a 0.1 mol/L solution of Nitric acid we will need to dilute 6.37 mL of 70 % HNO3 to a final volume with deionized (distilled) water. Transfer the prepared solution to a clean, dry storage bottle and label it. Never store solutions in a volumetric flask. All chemicals that you are unfamiliar with 6rDkTeZ.

calculate ph of hno3