Because Y removes protons at a pH greater than the pH of neutral water (7), it is considered a base. To describe how a buffer solution (either acidic or basic) can resist. Henderson-Hasselbalch Equation For Acid Buffer. Henderson-Hasselbalch Equation pH pKa + logA-1/HA -log(3.5x10-4) + log0.50/0.80 3.46 + (-0.40) 3.26 BACK TO MAIN PAGE. The principal objectives of the Henderson Hasselbalch equation include the following: To calculate the pH, pOH, H3O+ tot, OH- tot, H3O+ water, and OH- water in a solution containing a strong acid (base) given the initial concentration of the acid (base). ![]() For example, if you have a base Y with a pKa of 13, it will accept protons and form YH, but when the pH exceeds 13, YH will be deprotonated and become Y. pOH pKb + logSALT/BASE Henderson-Hasselbalch Equation for Base Buffer Use Henderson-Hasselbalch Equation to determine pH for 0.80M HF/0.50M NaF. Even a chemical ordinarily considered a base can have a pKa value because the terms "acids" and "bases" simply refer to whether a species will give up protons (acid) or remove them (base).On the other hand, the pKa value is constant for each type of molecule.It can be used for pH calculation of a solution containing pair of acid and. For example, concentrated vinegar (acetic acid, which is a weak acid) could have a lower pH than a dilute solution of hydrochloric acid (a strong acid). This is so called Henderson-Hasselbalch equation (or a buffer equation). Use the Henderson-Hasselbalch equation to calculate the pI. This is important because it means a weak acid could actually have a lower pH than a diluted strong acid. Calculate the pH of a weak acid solution of known concentration. pH depends on the concentration of the solution.The lower the pKa, the stronger the acid and the greater its ability to donate protons. ![]() The lower the pH, the higher the concentration of hydrogen ions.
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