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pay more attention in class. pH = pKa + log [A-]/[HA Im not helping you anymore
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How to prepare phosphate buffer pH 5.8?
preparation of 5.8 ph phosphate buffer
Prepare 5 M NaOH of pH 12?
na+oh +25=53 ph+poh=2.3
Do some alkaline have a pH greater then 9?
Yes. Some alkalis do have a pH above 9. e.g. 46% NaOH solution.
How do you prepare phosphate buffer of pH 7.5?
See the Related Links for "Columbia.edu: Phosphate buffer automatic calculator" to the bottom for the answer.
How can prepare 0.05mM from ZnSO4.7H2O?
You prepare 0.05mM from NaHC03 by first dissolving it. As you dissolve it in water, monitor the pH of the solution. The Internet does not list anything with the formula ZnSO4.7H20.
How do you prepare 20 mM tris hcl buffer pH 7.4?
to prepare 100ml of 100mM Trissolution: Mol wt of Tris=121.14121.14g in 1000ml ----> 1M12.11g in 100ml -------->1M1M=1000mM121.1g---->1000mM12.11g ----------->100mM1.211g in 100ml and 100mM Tris
How do you prepare tris-hcl buffer solution of 0.5M?
6g Tris HCl + 100ml dH2O, pH 6.8
How do you prepare sodium succinate buffer?
Prepared 0.5M succinic acid and 0.5 NaOH and adjusted pH to desired value
How do you prepare pH buffer soultion?
Decide on the concentration of the buffer, use 1L to be simple PH for your buffer should be within one pH unit from the pKa of the acid/conjugate base use Henderson Hasselbalch Equation pH = pKa + log ([Base]/[Acid]) For a 1 M buffer [Acid] + [Base] = 1
How much NaOH is needed to prepare 546 mL of solution with a pH of 10.00?
pH=10, so pOH=14-10=4 [OH]=10^-pOH [OH]=10^-4 [OH]=0.0001
How do you prepare 25mM sodium tartrate buffer pH 2.5?
Tartaric acid - 18.75 mM Sodium Tartrate Dihydrate - 6.25 mM pH of this mixture should be near 2.9, adjust pH down to 2.5 using HCl, and QS to 1 L by water.
How do you prepare phosphate buffer PH 6.8?
dissolve the 12 g of crystals of sodium phosphate in water to make 1oo ml
