The pH of the strong base is near 14 because the strong base is completely dissociated. The concentration of hydroxide ions is directly proportional to the pH of the solution. The concentration of the hydroxide ion is directly calculated from the concentration of a strong base. The relations...
Become a Study.com member to unlock this answer! Create your account View this answer HCl is a strong monoprotic acid. NaOH is a strong monoprotic base. The balanced reaction equation is: {eq}\rm HCl + NaOH \rightarrow H_2O +... See full answer below...
Calculate the pH of a buffer with different moles of a weak acid and conjugate base: 0.010 L of 0.10 M acetic acid, and 0.015 L of 0.10 M {eq}CH_{3}COONa {/eq}. pH of a Buffer Solution. Buffer solutions are pre...
Calculate the pH of a 0.0147 M aqueous solution of methylamine (Kb = 4.2 x 10-4) and the equilibrium concentrations of the weak base and its conjugate acid. Calculate the pH of a 0.350 M aqueous solution of nitrous acid...
For a 0.001 M solution of HCl, the pH is three, and the pOH is 11. You can also do the inverse calculation. Say you have a strong base which has a pH of 13. What is the pOH? \(\mathrm{14 = 13 +pOH}\) The pOH is thus: ...
According to my appendice attached in my Inorganic Chemistry, the Ksp value of Ca(OH)2 should be 5.26,then the saturated concentration should be at 0.01112mol/L or so since this is a strong base, its conc. then is 0.001mol/0.1L=0.01mol/L which is less than the saturated conc. Well,...
To calculate the pH of a weak acid, it is important to note that pH has no units, thus it is required to define it with H+ ion concentration.
Despite the fact that the salt solution isn't acidic at all, the pH drops considerably compared to the solution of the weak acid alone, simply because the metal and the anion form a very insoluble salt that precipitates, subtracting weak acid anions from the solution and forcing the ...
HA + H20 <--> H30++ A-, where A-is the conjugate base. Some acids are strong and dissociate completely while others are weak and only partially dissociate. You can measure the strength of an acid by its dissociation constant Ka, which is a ratio formed by dividing the concentration of ...
The Henderson-Hasselbalch equation can be used for finding the pH of a buffer solution after a strong base/acid is added. It also predicts the pH of a premade buffer after the addition of a strong acid/base. For the following NH4+/NH3 (pKa=9.25) buffer, calculate the pH of the ...