Ka, Kb, pH, pOH, H3O+ and OH- Calculations: ICE Tables (Acids and Bases Chemistry Problems).
This video explains Ka, Kb, pH and pOH calculations for weak acids and bases in chemistry. In this video we take a look at how to calculate pH, pOH, Ka and Kb step-by-step for chemistry problems involving weak acids and weak bases. In addition, we go through approximation to see if we can cancel out the variable, x. This video includes an abundance of practice problems and examples to work through. What are you waiting for? It's time to learn! :D ()()():)()()() 🍎 𝐑𝐞𝐝𝐨𝐱 𝐚𝐧𝐝 𝐄𝐥𝐞𝐜𝐭𝐫𝐨𝐜𝐡𝐞𝐦𝐢𝐬𝐭𝐫𝐲 𝐓𝐮𝐭𝐨𝐫𝐢𝐚𝐥𝐬: https://bit.ly/RedoxElectrochemistry ⚗️ 𝐂𝐡𝐞𝐦𝐢𝐜𝐚𝐥 𝐄𝐪𝐮𝐢𝐥𝐢𝐛𝐫𝐢𝐮𝐦 𝐚𝐧𝐝 𝐀𝐜𝐢𝐝-𝐁𝐚𝐬𝐞 𝐒𝐲𝐬𝐭𝐞𝐦𝐬 𝐓𝐮𝐭𝐨𝐫𝐢𝐚𝐥𝐬: https://bit.ly/EquilibriumAcidsBases 🧪 𝐂𝐡𝐞𝐦𝐢𝐬𝐭𝐫𝐲 𝟑𝟎 (𝐆𝐫𝐚𝐝𝐞 𝟏𝟐) 𝐓𝐮𝐭𝐨𝐫𝐢𝐚𝐥𝐬: https://bit.ly/Johnny_Chemistry30 Follow me for updates and behind the scenes: 📸 Instagram: https://bit.ly/3mPb2q7 ()()():)()()() Calculating Ka, Kb, pH, pOH, [H3O+] and [OH-] for weak acids and bases is a concept present in the Acid-Base Systems (Chemical Equilibrium) unit in Chemistry 30 (grade 12 level). ICE tables stand for: initial concentration, change in concentration and equilibrium concentration. ICE tables are only required for a weak acids and base problem when initial amounts or initial concentrations are given. Initial concentration + change in concentration = equilibrium concentration ( I + C = E). H2O(l) is a liquid, so we ignore it's concentration because it is mostly constant throughout the reaction. The equilibrium constant will not be Kc or Keq, but instead Ka for acids and Kb for weak bases. If the weak acid and base problem does not provide enough information to complete the chart with numbers, a variable must be used to represent I, C or E. As long as the problem gives the equilibrium constant value (Ka or Kb) - the variable can be solved by writing the equilibrium constant expression, plugging in the equilibrium constant value then plugging in the equilibrium concentrations and doing simple algebra calculations. ()()():)()()() Introduction - 0:00 Practice Problem (1, weak acid [H3O+]) - 0:07 Practice Problem (2, weak acid pH | quadratic formula) - 3:47 Practice Problem (3, weak acid pH) - 7:14 Practice Problem (4, weak acid Ka) - 10:09 Practice Problem (5, weak acid Ka) - 13:07 Practice Problem (6, weak base pOH ) - 15:27 Practice Problem (7, weak base pH) - 19:08 Polyprotic acid and base - 22:50 Remember Notes - 23:23 Conclusion - 23:34
This video explains Ka, Kb, pH and pOH calculations for weak acids and bases in chemistry. In this video we take a look at how to calculate pH, pOH, Ka and Kb step-by-step for chemistry problems involving weak acids and weak bases. In addition, we go through approximation to see if we can cancel out the variable, x. This video includes an abundance of practice problems and examples to work through. What are you waiting for? It's time to learn! :D ()()():)()()() 🍎 𝐑𝐞𝐝𝐨𝐱 𝐚𝐧𝐝 𝐄𝐥𝐞𝐜𝐭𝐫𝐨𝐜𝐡𝐞𝐦𝐢𝐬𝐭𝐫𝐲 𝐓𝐮𝐭𝐨𝐫𝐢𝐚𝐥𝐬: https://bit.ly/RedoxElectrochemistry ⚗️ 𝐂𝐡𝐞𝐦𝐢𝐜𝐚𝐥 𝐄𝐪𝐮𝐢𝐥𝐢𝐛𝐫𝐢𝐮𝐦 𝐚𝐧𝐝 𝐀𝐜𝐢𝐝-𝐁𝐚𝐬𝐞 𝐒𝐲𝐬𝐭𝐞𝐦𝐬 𝐓𝐮𝐭𝐨𝐫𝐢𝐚𝐥𝐬: https://bit.ly/EquilibriumAcidsBases 🧪 𝐂𝐡𝐞𝐦𝐢𝐬𝐭𝐫𝐲 𝟑𝟎 (𝐆𝐫𝐚𝐝𝐞 𝟏𝟐) 𝐓𝐮𝐭𝐨𝐫𝐢𝐚𝐥𝐬: https://bit.ly/Johnny_Chemistry30 Follow me for updates and behind the scenes: 📸 Instagram: https://bit.ly/3mPb2q7 ()()():)()()() Calculating Ka, Kb, pH, pOH, [H3O+] and [OH-] for weak acids and bases is a concept present in the Acid-Base Systems (Chemical Equilibrium) unit in Chemistry 30 (grade 12 level). ICE tables stand for: initial concentration, change in concentration and equilibrium concentration. ICE tables are only required for a weak acids and base problem when initial amounts or initial concentrations are given. Initial concentration + change in concentration = equilibrium concentration ( I + C = E). H2O(l) is a liquid, so we ignore it's concentration because it is mostly constant throughout the reaction. The equilibrium constant will not be Kc or Keq, but instead Ka for acids and Kb for weak bases. If the weak acid and base problem does not provide enough information to complete the chart with numbers, a variable must be used to represent I, C or E. As long as the problem gives the equilibrium constant value (Ka or Kb) - the variable can be solved by writing the equilibrium constant expression, plugging in the equilibrium constant value then plugging in the equilibrium concentrations and doing simple algebra calculations. ()()():)()()() Introduction - 0:00 Practice Problem (1, weak acid [H3O+]) - 0:07 Practice Problem (2, weak acid pH | quadratic formula) - 3:47 Practice Problem (3, weak acid pH) - 7:14 Practice Problem (4, weak acid Ka) - 10:09 Practice Problem (5, weak acid Ka) - 13:07 Practice Problem (6, weak base pOH ) - 15:27 Practice Problem (7, weak base pH) - 19:08 Polyprotic acid and base - 22:50 Remember Notes - 23:23 Conclusion - 23:34