btsarmyy
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I need help with this chemistry question:

The following problems are on neutralisation. Show whether each of the statements
below is true or false.

1 mol of HCL will neutralise:
(i) 5 dm3 of KOH(aq) of concentration 2.0 moldm-3
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wildone3
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HCl + KOH --> KCl + H2O (so 1:1 mole ratio)

moles = concentration x volume
moles = 5 x 2
moles = 10

so false as there would have to be equal moles of HCl for it to neutralise the KOH
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btsarmyy
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(Original post by wildone3)
HCl + KOH --> KCl + H2O (so 1:1 mole ratio)

moles = concentration x volume
moles = 5 x 2
moles = 10

so false as there would have to be equal moles of HCl for it to neutralise the KOH
Thank you so much! so for the answer to be true the need to have equal moles? not higher or not lower
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wildone3
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if HCl was higher then it would still neutralise KOH as it would be in excess. I should have said it must be equal to or higher :-)
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btsarmyy
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(Original post by wildone3)
if hcl was higher then it would still neutralise koh as it would be in excess. I should have said it must be equal to or higher :-)
thank you!!
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btsarmyy
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(Original post by wildone3)
if HCl was higher then it would still neutralise KOH as it would be in excess. I should have said it must be equal to or higher :-)
Sorry for asking so many questions😅but you know the ratio we work out say the equation is not balanced and you balance it , what are we looking for the ratios between?
example
1 mol of hcl will neutralise
250cm3 of na2co3 of a concentration 4 mol dm3-3

so i did:
250cm3 ----> 0.25dm3
Na2CO3 + 2HCL ----> 2NaCl + H2O + CO2
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wildone3
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So the moles of Na2CO3 in the reaction are:
moles = volume x concentration
moles = 0.25 x 4
moles = 1

According to the equation, two moles of HCl are needed to neutralise 1 mole of Na2CO3

therefore the ratio of Na2CO3 to HCl is 1:2
so for every 1 mole of Na2CO3 2 moles of HCl is needed

so I think if it is another true or false question then it would be false
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