PDF Use K*to Find The PH Of A Strong Base

4. Calculate the pH of 735 liters of a solution containing 0.34 moles of nitric acid (HNO3). J. Cruzan, 2013. Solutions to Web Exercises: Acids & Bases (1). 8. Calculate the pH and pOH of a solution that was made by adding 400 ml of water to 350 ml of a 5.0 x 10-3 M NaOH solution.The pH a 0.010 M HNO2 solution is <7, thus we have an acidic solution. what is the ph of an aqueous solution with the hydronium ion concentration [h3o+] = 2 x 10-14 m ?(Ka of HNO₂ is 4.5 × 10⁻⁴). Ph.D. University Professor with 10+ years Tutoring Experience.Determine the pH of a 0.010 M HNO₃ solution. What is the hydrogen ion concentration of an aqueous HCl solution that has a pH of 3.0? [H⁺] = 0.001 M.Click here to get an answer to your question Find the pH of a 0.010 M HNO2 solution. Now, we will calculate the amount of Hydronium [H3O+] in nitrous acid (HNO2), multiply the acid molarity by the degree of ionization, we will have:

find the ph of a 0.010 m hno2 solution. - Studyrankersonline

I'm getting pH 7.2 as near as makes no difference., with a square rooting but no polynomial equations. [OH-] - [H+] = [Na+] - [NO2-] = [HNO2] = [H+][NO2-] /Ka. I then make the approximation [NO2-] = [Na+] which, since we have salt of strong base and weak acid and we must be above pH 7 is good to better...Find Study Resources. This preview shows page 1 - 2 out of 2 pages. 4.Calculate the pH of a 0.10 M HNO2solution. Quiz 3Test Form ANovember 28, 20016.A 0.1 M aqueous solution of the salt NaHCO3is made.Chemistry Q&A Library Find the pH of a 0.010 M HNO2 solution. Want to see this answer and more? Experts are waiting 24/7 to provide step-by-step solutions in as fast as 30 minutes!*Вопросы Учеба и наука Химия Вычислите pH и pOH 0.01 М…

What is the pH of a solution of 0.300 M HNO₂ containing 0.170...

Substitute the E line into Ka expression for HNO2 and solvle for H^+. You have solutions of 0.200 M HNO2 and 0.200 M KNO2 (Ka for HNO2 = 4.00  10-4). A buffer of pH 3.000 is needed. What volumes of HNO2 and KNO2 are required to make 1 liter of buffered solution?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# As you know, molarity is defined as the number of moles of solute present in #10^3# #"mL"# of solution. For the nitric acid solution, you have.Two steps. Find molarity of nitric acid and need moles HNO3.Then find pH. pH = -log [H+ ion concentration] HNO3 is a strong acid, and because it is strong you can just plug 2.0M in for the H+ ion concentration and solve. PH of 0.010 M HNO3? Asked By Wiki User. Unanswered Questions.3) Find the pH of a solution that contains 0.0925 M nitrous acid (Ka = 4.5 x 10-4) and 0.139 M acetic acid (Ka = 1.8 x 10-5). Everett Community College Tutoring Center Student Support Services Program....of 0.036 M HNO2 solution (Ka= 4.47x10-4 ) So basically i know how to find the pH from the given Ka, but when it comes to this question idk how to incoporate the M of HNo2 given into finding the pH of the solution. Only the digits after the decimal are significant when you take the log of a number.

Data:Molar Mass of HNO2H = 1*1 = 1 amuN = 1*14 = 14 amuO = 3*16 = Forty eight amu------------------------Molar Mass of HNO2 = 1 + 14 + 48 = sixty three g/mol

M (molarity) = 0.010 M (Mol/L)

Now, since the Molarity and ionization constant has been provided, we will be able to find the degree of ionization, let us see:M (molarity) = 0.010 M (Mol/L)Use: Ka (ionization constant) = 

Now, we can calculate the quantity of Hydronium [H3O+] in nitrous acid (HNO2), multiply the acid molarity through the degree of ionization, we will have:

And finally, we will use the information found and put in the logarithmic equation of the PH, thus:

Data:log10(2.23) ≈ 0.34pH = ?

Formula:

Solving:

Note:. The pH <7, then now we have an acidic solution.

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