Concept explainers
In Example 16-9, rather than use the quadratic formul at o solve the quadratic c equation, we could have proceeded in the following way Substitute the value yielded by our failed assumption — x = 0.0010—into the denominator of the quadrati c equation: that is, use 10 00250 -0.00102 as the value of [CH2NH2 ] and solve for a new value of x Use this second value of x to re-evaluate [CH3NH3]: [CH2NH3] = 10 00250 -second value of x2 Solve the simple quadratic equation far a third value of x and so on. After three or four tnals. you will find that the value of x no longer changes This is thanswer you are seeking (a) Complete the calculation of the pH of 0.0250 M CH2NH2 by this method and show that the result is the same as that obtained by using the quadratic formula (b) Use this method to determine the pH of 0.500 M HCIO
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General Chemistry: Principles and Modern Applications (11th Edition)
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- For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.arrow_forward. The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted-Lowry acid-base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia. NH3. a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia. b. Write a chemical equation indicating how OH- behaves as a base in liquid ammonia.arrow_forwardTable 13-4 lists the stepwise Ka values for some polyprotic acids. What is the difference between a monoprotic acid, a diprotic acid, and a triprotic acid? Most polyprotic acids are weak acids; the major exception is H2SO4. To solve for the pH of a solution of H2SO4, you must generally solve a strong acid problem as well as a weak acid problem. Explain. Write out the reactions that refer to Ka1 and Ka2 for H2SO4. For H3PO4, Ka1 = 7.5 103, Ka2 = 6.2 108, and Ka3= 4.8 1013. Write out the reactions that refer to the Ka1, Ka2and Ka3equilibrium constants. What are the three acids in a solution of H3PO4? Which acid is strongest? What are the three conjugate bases in a solution of H3PO4? Which conjugate base is strongest? Summarize the strategy for calculating the pH of a polyprotic acid in water.arrow_forward
- Calculate the concentration of all solute species in each of the following solutions of acids or bases. Assume that the ionization of water can be neglected, and show that the change in the initial concentrations can be neglected, Ionization constants can be found in Appendix H and Appendix I. (a) 0.0092 M HCIO, a weak acid. (b) 0.0784 M C6H5NH2, a weak base. (c) 0.0810 M HCN, a weak acid. (d) 0.11 M (CH3)3N, a weak base. (e) 0.120 M Fe(H2O)62+ a weak acid, Ka=1.6107arrow_forwardEstimate the pH of a solution in which bromcresol green is blue and thymol blue is yellow. (See Fig. 14-8.)arrow_forwardExplain why equilibrium arrows are used in the ionization equations for some acids.arrow_forward
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