Science. Chemistry. Chemistry questions and answers. Calculate the pH of 100.00mL of 0.20 M HNO3 solution after 43.00 mL of NaOH 0.20 M have been added. What is the pH of a 0.25 M nitric acid (HNO3) solution? a.) 0.602 b.) 2.5 c.) 2.49 d.) 13.40 e.) none of these This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. 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.. 2 years ago Correct. That only applies at 25°C when the autoionization constant of water, Kw, is equal to 1.0 x 10^ (-14). If we use Jay's example here at 50°C, then pH + pOH should equal ~13.28. Hope that helps. Comment ( 9 votes) 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. 1) The equivalence point of an acid-base reaction (the point at which the amounts of acid and of base are just sufficient to cause complete neutralization). 2) The pH of the solution at equivalence point is dependent on the strength of the acid and strength of the base used in the titration. Let's calculate the pH of a strong acid solution. In this case, we're gonna do a 0.040M solution of nitric acid. Nitric acid is HNO3, and nitric acid reacts with water to form hydronium, H3O plus, and nitrate, NO3 minus, which is the conjugate base 2HNO3. pH=0.22 By definition, pH=-log_10[H_3O^+]we assume that nitric acid dissociates quantitatively. HNO_3(aq) +H_2O(l) rarr H_3O^+ +NO_3^(-) And so pH=-log_10(0. Question: 101 ved lumb 16.43 Calculate the pH of each of the following strong acid solu- tions: (a) 8.5 X 10-M HBr, (b) 1.52 g of HNO3 in 575 mL of solution, (c) 5.00 mL of 0.250 M HCIOdiluted to 50.0 mL, (d) a solution formed by mixing 10.0 mL of 0.100 M HBr with 20.0 mL of 0.200 M HCI. nch of the following strong acid solu-. Show transcribed The pH of the solution prepared by mixing NaOH and [tex]\rm HNO_3[/tex] has been 1.69 . The moles of NaOH can be given by: Moles = Molarity × Volume (L) Moles … calculate the ph of the solution resulting from the addition of 20 ml of 0.100 m naoh to 30 ml of 0.100 m - brainly.com NeDC2p.