Do you know what buffer capacity is? It's defined as the mols of strong acid or strong base that can be added to 1 L of a buffer solution and without changing the pH more than +/- 1.
The buffer capacity depends mostly upon two things.
1. The concn of base and acid components.
2. on the RATIO of the base/acid pair.
The maximum buffering capacity is delivered when the RATIO is 1.0. So you want C or D; those are the only ones with ratio of 1.0. Of the two which do you think would provide more capacity? The higher concn, of course.
Plan how you would make 100mL of a buffer solution with a pH of 10.80 to be made using only sodium carbonate, sodium hydrogen carbonate and water. You should specify the amount of sodium carbonate and sodium hydrogen carbonate
To create a 0.1 M carbonate buffer pH = 10.2. You choose to use a combination of HCO3- / CO32-. This buffer system has pKa = 9.9. a) Calculate how much you need to weigh in each of the sodium salts, NaHCO3 and Na2CO3, to create
Use the Bronsted-Lowry definitions to identify the two conjugate acid-base pairs in the following acid-base reaction: HCO3^- + S^2- HS^- + CO3^2- I got it. HCO3^- is the base in the pair with CO3^2-. S^2- is the acid in the pair
What arethe pH, pOH, and concentrations of CO3 2- and HCO3 - after 1.000 mL of 0.1500 M HCl is added to 100.0 mL of 0.0100-M sodium carbonate solution? ignore the added1% volume. CO3^-2 + H^+ ==> HCO3^- Calculate mols carbonate to
Assume that the normal blood buffer contains 0.00080 M carbonic acid and 0.0085 M hydrogen carbonate, the pKa = 6.35 for carbonic acid and the volume of blood in the body is 7.00 L. The blood pH, due to disruption is now 7.20.
I need to predict the acid/base reactions of sodium carbonate with HCl, CH3COOH, NH3, and NaOH. I'm stuck, when I'm writing out the ions to find the strongest acid and base, does the NaHCO3 become Na and HCO3, or N, H, and CO3?
Write the balanced net ionic equation for the following reaction and determine the conjugate acid-base pairs. HNO3(aq)+Li2CO3(aq)LiNo3(aq)+LiHCO3(aq) Which component in the net ionic equation is the acid, the base, the conjugate
The pH of a buffer can be predicted using the Hendersen-Hasselbach equation: pH=pKa+ log([conjugate base][conjugate acid]) The choice of the conjugate acid-base pair (as you did in the previous questions) determines the pKa value
Need help with my pH calculations? 1) 0.10 mol of solid sodium hydrogen carbonate and 0.20 mol of solid sodium carbonate are dissolved in the same beaker of water, transferred to a volumetric ﬂask and made to 250.0 mL. The Ka
Not sure if i posted this but Need help with my pH calculations? 0.10 mol of solid sodium hydrogen carbonate and 0.20 mol of solid sodium carbonate are dissolved in the same beaker of water, transferred to a volumetric ﬂask and