say for example the equilibrium I2(aq)+H2O(l)-----HOI(aq)+I(aq)+H(aq)
Think Lechatlier principle... addition of NaOH will cause the H ions to react with the OH ions to cause more water (more reactants) increase in reactants shifts the equilibrium in the FORWARD direction to form MORE H+ to restore the equilibrium
A base or alkaline substance lowers the H (hydrogen ion) concentration in a solution. Bases can accept or remove hydrogen ions from the solution, increasing the concentration of OH- ions and thereby reducing the concentration of H+ ions. Examples of bases include sodium hydroxide (NaOH) and ammonia (NH3).
The addition of sodium hydroxide (NaOH) increases the pH of a solution by releasing hydroxide ions (OH-) which combine with hydrogen ions (H+) to form water. However, the addition of sodium ions (Na+) alone does not directly impact the pH of a solution.
No, NaOH (sodium hydroxide) does not contain H+ ions. When NaOH dissolves in water, it dissociates into Na+ and OH- ions, with OH- being the hydroxide ions that can accept H+ ions to form water in a chemical reaction.
In a base, the concentration of hydrogen ions (H+) decreases as they accept protons to form hydroxide ions (OH-). This leads to an increase in the concentration of hydroxide ions, resulting in a higher pH and a more basic solution.
The balanced chemical equation for the reaction is H₂C₃H₂O₄ + 2NaOH → Na₂C₃H₂O₄ + 2H₂O. By stoichiometry, 1 mol of malonic acid reacts with 2 mol of NaOH. From the given data, the concentration of the malonic acid solution can be calculated to be 0.133 M.
pH would decrease since H+ concentration increases, while pOH would increase since OH- concentration decreases. But pH would always be above 7 and pOH would always be below 7 since H+ will never be equal to OH- [OH-] would be always be greater than [H+] in any solution of NaOH , however dilute. Also remember pH + pOH =14, thus if pH decreases then pOH increases. Thanking you Yours Rajiv
The concentration of hydrogen ions in a 0.0010M aqueous solution of NaOH is 1.0 x 10^-11 mol/L, as NaOH dissociates in water to form Na+ and OH- ions. In this process, there are no hydrogen ions produced.
The amount of NaOH needed to raise the pH from 8 to 10 depends heavily on the conditions. The amount of NaOH needed will increase as the volume of the solution increases. Even more importantly, buffers can stabilize the pH significantly. If buffers are presently, the pH change will be much more gradual, and more NaOH will be required.
The concentration of H+ ions in a solution determines its acidity; the higher the concentration of H+ ions, the lower the pH. The concentration of OH- ions in a solution determines its alkalinity; the higher the concentration of OH- ions, the higher the pH. pH is a logarithmic scale that represents the concentration of H+ ions in a solution.
Use the working definition of pH used in General Chemistry classes: pH = -log([H+]) and the equilibrium constant for ionization of water: [H+][OH-]=10-14 (Here [] denotes concentration in Molarity) For moderate concentrations of NaOH (like 10-4-ish M and up, we can neglect the [OH-] from the actual ionization of water (since 10-7 is the maximum this concentration could be, when the NaOH concentration is 0, and even this is much less than the concentration of NaOH). Then we can say: 10-14=[H+][OH-]=[H+][NaOH] and then pH=-log[H+]=-log(10-14/[NaOH]) Just as an example, a 0.5 M solution has a pH of approximately -log(10-14/0.5) which is about 13
In a 0.25M solution of NaOH, the concentration of hydroxide ions (OH-) is also 0.25M. This is because NaOH dissociates completely in water to form Na+ and OH- ions. OH- represents the hydroxide ion in solution.
A base or alkaline substance lowers the H (hydrogen ion) concentration in a solution. Bases can accept or remove hydrogen ions from the solution, increasing the concentration of OH- ions and thereby reducing the concentration of H+ ions. Examples of bases include sodium hydroxide (NaOH) and ammonia (NH3).
The addition of sodium hydroxide (NaOH) increases the pH of a solution by releasing hydroxide ions (OH-) which combine with hydrogen ions (H+) to form water. However, the addition of sodium ions (Na+) alone does not directly impact the pH of a solution.
2H - C - H + NaOH ------> H- C - O -Na + CH3 - OH
No, NaOH (sodium hydroxide) does not contain H+ ions. When NaOH dissolves in water, it dissociates into Na+ and OH- ions, with OH- being the hydroxide ions that can accept H+ ions to form water in a chemical reaction.
When NaOH is added to water, it dissociates into Na+ and OH- ions. The increase in hydrogen concentration is due to the OH- ions reacting with water to form more H2O molecules, shifting the equilibrium towards formation of additional H+ ions. This suggests that NaOH is a strong base that can increase the hydrogen ion concentration in a solution.
acids are substances that release their hydrogen ion(s) while bases grab hydrogen ions to themselves. SO, adding acids will increase the H+ concentration while adding bases will decrease the H+ concetration of the solution. This would be considered a direct effect.