In a titration, 45.0 mL of KOH is neutralized by 75.0 mL of 0.30 M HBr. How much KOH is in 1.0 liter of the KOH solution?
Answer (2)
In a titration , 45.0 mL of KOH is neutralized by 75.0 mL of 0.30M HBr. 0.5 moles o f KOH are is in 1.0 liter of the KOH solution.
What is mole?
A **mole **is just a measuring scale. In fact, it is one of the Worldwide System of Units' (SI) seven base units . When already-existing units are insufficient, new ones are created. The levels at which chemical reactions frequently occur exclude the use of grammes, but utilising absolute numbers of atoms, molecules, or ions would also be unclear.
To fill this gap between extremely small and extremely huge numbers, scientists created the mole. A **mole **was once defined as the volume of something that consists of the same proportion of particles as 12.000 grammes of carbon-12.
KOH + HBr → KBr + H2O
0,3 moles of HBr in 1000ml
x moles of HBr in 75ml
x = 0,0225 moles of HBr
1 mole of KOH = 1 mole of HBr
0,0225 moles of HBr = 0,0225 moles of KOH
0,0225 mole of KOH in 45ml
x moles of KOH in 1000ml
x = **0.5 moles **of KOH
Therefore, **0.5 moles **of KOH are is in 1.0 liter of the KOH solution.
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The titration of 45.0 mL of KOH with 75.0 mL of 0.30 M HBr shows that there are 0.5 moles of KOH in 1.0 liter of KOH solution. This is derived from the stoichiometry of the reaction where 1 mole of KOH reacts with 1 mole of HBr. Therefore, using the volume relationships, we find that the concentration is 0.5 moles in a liter.
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