The pH Titration of a Weak Monoprotic Acid A pH titration is an important tool in analytical chemistry since it allows the experimenter to better understand and the titration process and provides important information regarding the nature of the acid and base reacted. Conjugate bases of strong acids are ineffective bases. Problem #1: Acetic acid is a weak monoprotic acid with K a = 1.77 x 10¯ 5.NaOH(s) was gradually added to 1.00 L of 0.0179 M acetic acid. After the addition of 10.6 milliliters of base, a pH of 5.65 was recorded. Strong acids has pK a values of less than about −2; the dissociation of a strong acid is effectively complete such that concentration of the undissociated acid is too small to be measured. (Assume no volume change occurs.) what is the percent ionization of a 0.169 M solution of this acid? How? Answer: pH = 2.808 Weak Acid Equilibria: Fraction of Dissociation The fraction of dissociation, α (Greek: alpha), of a weak acid HA refers to the fraction of HA in the dissociated form A-, i.e. * HCl is a strong, monoprotic acid. Furthermore, a … A 0.682 gram sample of an unknown weak monoprotic organic acid, HA was dissolved in sufficient water to make 50 milliliters of solution and was titrated with a 0.135 molar NaOH solution. An acid is a molecule or ion capable of donating a proton (hydrogen ion H +) (a Brønsted–Lowry acid), or, alternatively, capable of forming a covalent bond with an electron pair (a Lewis acid).. A weak acid has a pK a value in the approximate range −2 to 12 in water. Sulfuric acid is a strong, diprotic acid. Hydronium ion H3O+ H2O 1 0.0 Iodic HIO3 IO3-1.6 x 10-1 0.80 Oxalic (1) -2H2C2O4 HC2O4-5.9 x 10 1.23 Sulfurous (1) H2SO3 HSO3-1.54 x 10-2 1.81 (pK a = 3.745). (a) Calculate the pH of the solution after the addition of 0.0107 mol of NaOH(s). The charge of a monoprotic acid is always one higher before it gives away the hydrogen ion. Items to remember about conjugate acid-base pairs: • The conjugate acid of a weak base is a weak acid and the conjugate base of a weak acid is a weak base. Percent Dissociation. A monoprotic acid is one that has one acidic hydrogen atom per molecule. The degree of ionization for a weak monoprotic acid HA is given by the expression ( [H+]eq/[HA]0 ) * 100. Interestingly, phosphoric acid is triprotic, but only the first two protons are strong acids, so with weak bases it is diprotic, and it only forms two moles of [math]H_3O^+[/math] when dissolved in water. pK a values for strong acids can, however, be estimated by theoretical means. A 0.32 M solution of phenol, which is a weak monoprotic acid, has a pH of 5.22. HINT: You must first determine K a from pK a. Some examples of each scenario will be given. Whether an acid is monoprotic has nothing to do with how strong it is. The first category of acids are the proton donors, or Brønsted–Lowry acids.In the special case of aqueous solutions, proton donors form the hydronium ion H 3 O + and are known as Arrhenius acids. Organic acid (carboxylic acid) - an acid (except carbonic acid, H 2 CO 3 (aq)) containing carbon, oxygen, and hydrogen atoms.An organic acid has a carbon backbone and a carboxyl group (-COOH).. Carbonic acid is a weak, diprotic acid. • For any conjugate acid-base pair, K aKb=Kw, where Ka is the acid dissociation constant for the weak acid, and K b is the base hydrolysis constant for the conjugate base. the Ka of a monoprotic weak acid is 2.28 x 10^-3. The following key statement is common sense: Any acid with only one hydrogen atom is monoprotic. This is called the (A) ionization and is a measure of acid strength. A diprotic acid has two; a triprotic acid has three; and so on. Acetic acid (vinegar) is a weak, monoprotic acid. (A) - percent. 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