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How much HCl is needed to neutralise NaOH?
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+ Sodium hydroxide
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Mel B.
How much HCl is needed to neutralise NaOH?
Since HCl is a strong acid and sodium hydroxide is a strong base they dissociate 100%. Both have a normality of one. So there is a 1 to 1 ratio of hydronium and hydroxide ions in solution. Because of this whatever amount of acid to add to a solution, an equal amount of sodium hydroxide would cause a neutralization. That is adding 10 mL of a one normal solution of HCl just requires 10 mL of a one normal solution of NaOH to bring the pH back to 7, assuming there are no buffers present.
Since HCl is a strong acid and sodium hydroxide is a strong base they dissociate 100%. Both have a normality of one. So there is a 1 to 1 ratio of hydronium and hydroxide ions in solution. Because of this whatever amount of acid to add to a solution, an equal amount of sodium hydroxide would cause a neutralization. That is adding 10 mL of a one normal solution of HCl just requires 10 mL of a one normal solution of NaOH to bring the pH back to 7, assuming there are no buffers present.
Here is the reaction equation for the neutralization. One mole of NaOH reacts in equal 1:1 equivalents ratio with one mole of HCl.
Therefore, for example, if the NaOH is 10ml of 6N solution, either 10ml of 6N HCl is needed, 30ml of 2N HCl or 60ml of 1N HCl would be needed.
In a neutralization reaction the concentration is expressed as normality, N, that is, molar equivalents per L. It is similar to molarity, M, where it is in moles per L. 1000meq = 1eq 1000ml = 1L 1000mmol = 1 Mol
Here is the reaction equation for the neutralization. One mole of NaOH reacts in equal 1:1 equivalents ratio with one mole of HCl.
Therefore, for example, if the NaOH is 10ml of 6N solution, either 10ml of 6N HCl is needed, 30ml of 2N HCl or 60ml of 1N HCl would be needed.
In a neutralization reaction the concentration is expressed as normality, N, that is, molar equivalents per L. It is similar to molarity, M, where it is in moles per L. 1000meq = 1eq 1000ml = 1L 1000mmol = 1 Mol
Since HCl is a strong acid and sodium hydroxide is a strong base they dissociate 100%. Both have a normality of one. So there is a 1 to 1 ratio of hydronium and hydroxide ions in solution. Because of this whatever amount of acid to add to a solution, an equal amount of sodium hydroxide would cause a neutralization. That is adding 10 mL of a one normal solution of HCl just requires 10 mL of a one normal solution of NaOH to bring the pH back to 7, assuming there are no buffers present.
Since HCl is a strong acid and sodium hydroxide is a strong base they dissociate 100%. Both have a normality of one. So there is a 1 to 1 ratio of hydronium and hydroxide ions in solution. Because of this whatever amount of acid to add to a solution, an equal amount of sodium hydroxide would cause a neutralization. That is adding 10 mL of a one normal solution of HCl just requires 10 mL of a one normal solution of NaOH to bring the pH back to 7, assuming there are no buffers present.
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Here is the reaction equation for the neutralization. One mole of NaOH reacts in equal 1:1 equivalents ratio with one mole of HCl.
Therefore, for example, if the NaOH is 10ml of 6N solution, either 10ml of 6N HCl is needed, 30ml of 2N HCl or 60ml of 1N HCl would be needed.
In a neutralization reaction the concentration is expressed as normality, N, that is, molar equivalents per L. It is similar to molarity, M, where it is in moles per L. 1000meq = 1eq 1000ml = 1L 1000mmol = 1 Mol
Here is the reaction equation for the neutralization. One mole of NaOH reacts in equal 1:1 equivalents ratio with one mole of HCl.
Therefore, for example, if the NaOH is 10ml of 6N solution, either 10ml of 6N HCl is needed, 30ml of 2N HCl or 60ml of 1N HCl would be needed.
In a neutralization reaction the concentration is expressed as normality, N, that is, molar equivalents per L. It is similar to molarity, M, where it is in moles per L. 1000meq = 1eq 1000ml = 1L 1000mmol = 1 Mol
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VOTE