How do you calculate the Ka of an acid? + Example - Socratic
2017年7月10日 · What is the equation for finding the equilibrium constant for a chemical reaction? What is the equilibrium constant for the weak acid KHP? Consider this equilibrium: I2(s) + H2O(l) ⇌ H+(aq) + I-(aq) + HOI(aq).
What is the Ka of a strong acid like HCl? - Socratic
2016年8月23日 · The approximate value of pKa is -7 for HCl. Hydrochloric acid is a strong acid and it is considered to completely dissociate in water under the following equation: HCl(aq)+H_2O(l)->H_3O^(+)(aq)+Cl^(-)(aq) The equilibrium constant K_a is written as: K_a=([H_3O^+][Cl^-])/(HCl] Since the acid dissociates completely, the concentration of …
What is the equilibrium constant for the weak acid KHP?
2015年1月14日 · Potassium hydrogen phthalate ("KHP") has the molecular formula "C"_8"H"_5"KO"_4 and is known to be a weak acid.
What is Ka in chemistry? - Socratic
2016年9月28日 · This is the acid dissociation constant, which quantifies the extent of acid dissociation in a solvent, typically water. An acid, HA, undergoes the following equilibrium in water: HA(aq) + H_2O(l) rightleftharpoons H_3O^+ + A^- For strong acids, this equilibrium lies strongly to the right; and for weak acids, the equilibrium lies to the left (as written, i.e. as we …
How can I calculate Ka of #NH_4^+#? - Socratic
2014年12月6日 · NH_4^+ is a weak acid, which would give us an idea if not about the actual value, then at least about its dissociation constant's dimension. Knowing that the ammonium ion (NH_4^+) is a weak acid, we should expect K_a to be less than 1. That is, a very small quantity of products ( ammonia and hydronium cation ) will be formed, the reaction favoring the reactans …
How would you rearrange the Henderson–Hasselbalch equation
2016年1月2日 · The most common form of the Hendeson - Hasselbalch equation allows you to calculate the pH of a buffer solution that contains a weak acid and its conjugate base. #color(blue)("pH" = pK_a + log( (["conjugate base"])/(["weak acid"])))" "# Here #pK_a# is equal to . #color(blue)(pK_a = - log(K_a))" "#, where . #K_a# - the acid dissociation constant ...
The K_a for HCOOH is 1.78*10^-4. What would be the expected
2018年4月30日 · The concentration of the hydronium ion, or [H_3O^+], is 1.3*10^-2color(white)(l)M. For this, problem, we will use an ICE table. To start, we need the net ionic equation for the reaction of HCOOH, formic acid, with H_2O, water. HCOOH(aq)+H_2O(l)rightleftharpoonsH_3O^"+"(aq)+HCOO^"-"(aq) Now, we can create our …
pH, pKa, Ka, pKb, Kb - Organic Chemistry - Socratic
pH describes the acidity of a solution. pKa and pKb are the logarithmic acid and base dissociation constants, respectively. Ka and Kb are the acid and base dissociation constants which serve as quanitified measurements of the strength of an acid in solution, respectively.
What is the equation for the acid ionization constant of HNO3?
2018年7月3日 · K_a = ([H^+][NO_3^-])/[HNO_3] The equation for ionization of nitric acid, HNO_3 can be written as HNO_3(aq) -> H^+(aq) + NO_3^-(aq) From the equation, the acid ...
Buffer Calculations - Chemistry - Socratic
Ka for HF is 3.5x10^-4 How would you use the Henderson–Hasselbalch equation to calculate the pH of each a solution that contains 1.40% C2H5NH2 by mass and 1.18% C2H5NH3Br by mass? How would you use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution that is 0.27 M in formic acid (HCO2H) and 0.50 M in sodium formate ...