Please help! Write the formula for the conjugate base of ...

I really struggled with understanding titrations until I worked my way through this theoretical titration of carbonic acid with NaOH, so I figured I'd post it here in case anyone else needed help! This can also apply to titration of amino acids!
Here are the key ideas to know:
• Essentially, the number of protons you have to neutralize = the number of half-equivalence points = the number of full equivalence points
• The full equivalence point is where you’ve COMPLETELY removed a proton and you have 100% the resulting deprotonated conjugate base
• The half-equivalence point is the same thing as the buffering region! Thus, at a half equivalence point, you have a 50:50 mixture of an acid and its deprotonated conjugate base!
• M1n1V1 = M2n2V2 (memorize this equation like your life DEPENDS on it lmao); this equation will tell you the conditions at the equivalence point of the titration, which is when you've completely neutralized all your acid!
– M = molarity
– n = the number of "equivalents" (e.g., for NaOH, n = 1 because it gives 1 equivalent of base; for H2SO4, n = 2 because it gives 2 equivalents of acidic protons)
– V = volume (in mL or L)
☆ Say you're performing the titration of 50 mL 0.1 M H2CO3 with 0.2 M NaOH
• Use your formula; you should get that you require 50 mL of NaOH to completely neutralize all your H2CO3. 50 mL NaOH is equivalent to two equivalents of NaOH.
• What does "completely neutralized" H2CO3 look like? At the equivalence point, you've stripped off BOTH of H2CO3's protons, leaving you with CO3(2-)!
• Since you know 50 mL NaOH strips off BOTH protons, you can thus infer that 25 mL NaOH only strips off ONE proton, giving you HCO3-!
With this in mind, let's work through the titration:
1) At very acidic pH values, H2CO3 exists predominantly at 100% H2CO3
2) When you have added 0.5 equivalents of NaOH (12.5 mL), H2CO3 exists as a 50:50 mixture of HCO3- and H2CO3! This is the FIRST half-equivalence point (buffering region)! Remember what a buffer is? A buffer is a 50:50 mixture of either an acid and a salt containing its conjugate base (e.g., acetic acid and sodium acetate) or a 50:50 mixture of a base and a salt containing its conjugate acid (e.g., ammonia and ammonium chloride)! This is exactly what you have at the half-equivalence point: a buffer! "50:50" = "half and half" = "half-equivalence point"! The half-equivalence point/buffering region would appear as a flat line on a titration curve
3) When you have added 1 equivalent of NaOH (25 mL), H2CO3 exists as 100% HCO3-! This is the FIRST full equivalence point, signalling that you've COMPLETELY removed the first proton from H2CO3 and now ONLY have HCO3-! Again, there is no 50:50 mixture, so this is a FULL equivalence point, NOT a half-equivalence point! This would appear as a sharp vertical line on a titration curve!
4) When you have added 1.5 equivalents of NaOH (37.5 mL), you will have a 50:50 mixture of HCO3- and CO3(2-)! This is the SECOND half-equivalence point/buffering region! Again, it appears as a flat line!
5) When you've added 2 equivalents of NaOH (50 mL), you will have a 100% mixture of CO3(2-)! This is the SECOND and FINAL equivalence point! Again, it appears as a sharp vertical line!
And that's it! As long as you understand the equation and the concept of equivalents, you should be golden! I really hope this helps out anyone who needs it. Good luck!

formula for conjugate base of h2co3 video

The conjugate base of bicarbonate, HCO 3- is carbonate, CO3 2-. HCO3- is a conjugate acid, H 2 CO 3. Log in or register to post comments; Similar Questions. What is the conjugate acid of base HCO3- ? The Ka for HCO3- is 4.7 x 10^-11, what is the conjugate base and its Kb? What is the conjugate base of HF? What is the conjugate base of acid HClO4 ? What is the conjugate base of acid H2S ? What ... HCO3- (known as bicarbonate) is the conjugate base of H2CO3, a weak acid, and the conjugate acid of the carbonate ion. HCO3- acts as a base when mixed with a compound that is more acidic than itself (larger Ka) and as an acid when mixed with a compound that is more basic than itself (smaller Ka). Write the formula of the conjugate base for each of the following acids: HCO3-1 HPO4-2 H3O+ HSO4-Co3-2 PO4-3 H2O SO4-2 . Write the formula for the conjugate acid for each of the following bases: SO4-2 OH-1 HS-1 ClO2-1. HSO4-H2O H2S HCLO2. Identify the stronger acid in each pair: NH4+ or H3O+ H2SO4 or HCN H2O or H2CO3. H3O+ H2SO4 H2CO3. Identify the weaker acid in each pair: HNO3 or HCO3-HSO4 ... So H2CO3 (acid) = HCO3- + H+ and the HCO3- is your conjugate base. Same works for bases and conjugate acids. Names you should just memorize for any irregularities Conjugated bases always have one proton less than its (conjugated) acids:So the conjugated base of carbonic acid ( H2CO3 ) is: hydrogen carbonate, formula HCO3- acid base base acid. here H2CO3 and HCO3- are conjugate acid-base pair as are H2O and OH-b) HCl + H 2 PO 4-<-----> Cl - + H 3 PO 4. HCl transfers a proton (H+ ion) to H 2 PO 4- and form Cl - and H 3 PO 4, now Cl - can accept a proton donated by H 3 PO 4 .so the above equation is; Answer and Explanation: The conjugate base contains one less H than its corresponding acid and 1 more negative charge than its corresponding acid. So, the conjugate base for H2CO3 H 2 C O 3 HCO− 3... Write the formula of the conjugate base for acid H2CO3. Express your answer as an ion. 2. Calculate the [OH−] of each aqueous solution with the following [H3O+]: stomach acid, 4.5×10−2M. Express your answer using two significant figures. urine, 6.0×10−6M. Express your answer using two significant figures. orange juice, 2.2×10−4M. Express your answer using two significant figures ... Write the formula for the conjugate base of each of the following acids. HBr (express your answer as an ion) H2CO3 (express your answer as an ion) Answer Save. 3 Answers. Relevance. Greg G. Lv 5. 1 decade ago. Favorite Answer. The conjugate base of an acid results simply from the loss of a proton. A proton is a hydrogen(H) atom. The loss of a proton results in a negative charge. For HBr we get ... Conjugated bases always have one proton less than its (conjugated) acids:So the conjugated base of carbonic acid ( H2CO3 ) is: hydrogen carbonate, formula HCO3-

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Conjugate acids and bases - YouTube

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Please help! Write the formula for the conjugate base of ...

formula for conjugate base of h2co3

formula for conjugate base of h2co3 - win

Titration Overview

formula for conjugate base of h2co3 video

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Conjugate acids and bases - YouTube