Multiple Choice
In the balanced chemical equation for the reaction between ethylenediaminetetraacetic acid (EDTA) and calcium ion (Ca^{2+}), what is the mole ratio of EDTA to Ca^{2+}?
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3. Chemical Reactions
Stoichiometry
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How many milliliters of 0.100 M HNO3 are required to completely neutralize 25.0 mL of 0.150 M NaOH?
A
50.0 mL
B
16.7 mL
C
25.0 mL
D
37.5 mL
Verified step by step guidance1
Write the balanced chemical equation for the neutralization reaction: \(\mathrm{HNO_3 + NaOH \rightarrow NaNO_3 + H_2O}\). This shows a 1:1 mole ratio between HNO3 and NaOH.
Calculate the moles of NaOH present using the formula: \(\text{moles} = M \times V\), where \(M\) is molarity and \(V\) is volume in liters. For NaOH, convert 25.0 mL to liters and multiply by 0.150 M.
Since the reaction ratio is 1:1, the moles of HNO3 required to neutralize the NaOH are equal to the moles of NaOH calculated.
Use the moles of HNO3 and its molarity (0.100 M) to find the volume of HNO3 needed: \(V = \frac{\text{moles}}{M}\). This volume will be in liters.
Convert the volume of HNO3 from liters to milliliters by multiplying by 1000 to get the final answer.
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