A student has a solution of 0.05 ammonium chloride. The Ka for ammonium is 5.7x10^-10. Using the systematic approach, solve for the concentrations of H30+, NH3, and NH4+. (Analytical Chemistry)
concentration of NH4Cl = 0.05 M
Ka = 5.7 x 10^-10
NH4+ + H2O ------------> NH3 + H3O+
0.05 0 0
0.05 - x x x
Ka = x^2 / 0.05 - x
5.7 x 10^-10 = x^2 / 0.05 - x
x = 5.34 x 10^-6
[H3O+] = 5.34 x 10^-6 M
[NH3] = 5.34 x 10^-6 M
[NH4+] = 0.05 M
A student has a solution of 0.05 ammonium chloride. The Ka for ammonium is 5.7x10^-10. Using...
Calculate the hydronium ion concentration and pH in a 0.92 M solution of ammonium chloride. Ka NH4+ = 5.6x10^-10
we consider an ammonium solution with a concentration of 0.05 mol / L 1) Write the equation of acidic basic equilibrium between NH4 + ammonium ions and water 2) Express literally the acidity constant KA of this equation. 3) Make the progress table showing the progress of the reaction x and give the expression of the acidity constant KA as a function of x. 4) Establish the second degree equation to determine the concentration of H3O + ions 5) Calculate...
Data Table 2. Solutions of Ammonium lon- Ammonia Solution [NHaCl], M Acid, base, or neutral? Experimental pH NH3], M 0.10 1.0 0.050 0.50 0 0 0 0.05 0.50 0.10 6.23 Acid cid Base Bage base .5 lo. && The concentrations of [NHaCI] and [NH3] will need to be calculated using the ICE-box method before they are entered in the table below. Show one representative calculation. (Attach an additional sheet of paper to this lab if necessary.) 2. Table 3. Determining...
What is the pH of a 0.250 M aqueous solution of ammonium chloride (NH4+Cl-)? Kb (NH3) = 1.2 × 10-5 A. 5.04 B. 4.95 C. 4.77 D. 4.84 E. 6.26
Ka of (NH4)+ : 5.70x10^-10
Ka of Piperidinium ion: 7.50x10^-12
Ka of ethyl ammonium ion: 3.18x10^-10
Ka of anilinium ion: 2.51x10^-5
What is the pH of a solution that is (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match.) a prepared by dissolving 4.30 g of (NH4),S04 in water, adding 100.0 mL of...
(25 pts) Solve for the time-dependent concentration of ammonium chloride based on the following reaction equation. Assume that the reaction rate constants and the concentrations of ammonia and hydrogen chloride are constant. Assume an initial concentration of ammonium chloride of 0.5mM. Be sure to solve for the constants. NH3+HCl NH4CI Reaction: a. (5 pts) Write the reaction rate equation for NH2C b. (5 pts) Write the differential equation in our standard form (+A -y = B) dx c. (5 pts)...
Calculate the approximate pH of an aqueous solution of ammonium chloride, NH4Cl , 0.03 M, and sodium acetate, CH3COONa, 0.12 M at 25°C. (Note: consider one decimal place for the pH answer.) pKa NH4+/NH3 = 9.24 pKa CH3COOH/CH3COO- = 4.76
A buffer solution consists of 0.00300 M ammonia (NH3) and 0.00500 M ammonium chloride (NH4Cl). What is the change in pH when 0.00100 moles of NaOH are added to one litre of the solution without any change in volume? The pKa of NH4+ is 9.24.
What is the amount of ammonium chloride that has to be dissolved in 190 mL of 0.189 M NH3(Kb= 1.8×10‒5) to make it a buffer with a pH of 8.96, in grams? A mixture contains 0.250 M benzoic acid, a monoprotic acid (Ka = 6.28 × 10‒5), and 0.400 M sodium benzoate. How many mL of a HCl solution whose pH is 0.523 should be added to 500 mL of this buffer to change its pH from what it is...
Question 10 0/5 points A buffer solution is made such that the initial concentrations of lactic acid (HC3H5O3) and the lactate ion (C3H503) are both 0.600 M. What is the resulting pH if 0.020 mol of hydrochloric acid is added to 0.500 L of the buffer solution? (The Ky of HC3H5O3 is 1.4 x 10" 4.) HINT: Use your RICE chart! [A-] Note: pH = pka + log [HA] Ka x Ky = Kw = 1.0 x 10-14 2.92 3.80...