AcidBase Chemistry With No Calculator
 by
 Aug 06, 2018
 MCAT Blog, MCAT Chemistry
The HendersonHasselbalch Equation In Action On The MCAT
Consider the following problem: we mix nitrous acid, which has a K_{a} of 4.0 × 10^{4}, with its conjugate base at a 4:1 acidbase ratio. What is the pH of the resulting buffer solution? This simplesounding problem contains several useful teaching points for handling acidbase chemistry with no calculator.
In this blog post, we’ll work through the problem systematically, drawing attention to some key “tricks” that you can apply to solve it, and then discuss how you can use these tricks to set yourself up for success on the MCAT chemistry questions.
Setting Up The Problem
The first thing to figure out for this question is how to approach solving it. As soon as you see that the question is asking about the ratio of a weak acid to its conjugate base, you should immediately think of the HendersonHasselbalch equation, which relates pH, pK_{a}, and the ratio of [HA] (an acid) to [A–] (its conjugate base) as follows:
pH = pK_{a} + log[A–]/[HA]
Calculating The pK_{a}
This question gives us the acidbase ratio and the K_{a}, so our first task is to translate that information into the form we need for the HendersonHasselbalch equation. The first issue we need to deal with is going from K_{a} to pK_{a}. Recall that in acidbase chemistry, pX means –log[X]: pH = –log{H+], pOH = –log[OH–], and so on. Therefore, to calculate the pK_{a}, we need to calculate –logK_{a}, which is –log(4.0 × 10^{4}), based on the information in the question. This may seem like a daunting mathematical task, but there’s a neat trick we can use to estimate this, given a value in scientific notation of N × 10^{M}:
p(N × 10^{M}) = (M1).(10N)
Let’s walk through this trick a little bit more carefully to see how it works. Since a logarithm in general corresponds to the power of 10, M will be the most important number for calculating the magnitude of the pK_{a} value. We can use the question information to see this. If the K_{a} was 1.0 × 10^{4}, the pK_{a} would just be 4, based on a straightforward definition of what a negative log is. If the K_{a} was 1.0 × 10^{3} (which equals 10 × 10^{4}), the pK_{a} would be 3. In this problem, we’re given a K_{a} of 4.0 × 10^{4}, which is somewhere between 1.0 × 10^{4} and 1.0 × 10^{3}, so the pK_{a} must be somewhere between 3 and 4.That’s what the (M1) term in our shortcut means.
The next question is where does the pK_{a} lie in that interval: is it closer to 3 or to 4? This of course depends on whether the K_{a} is closer to 1.0 × 10^{4 }or 1.0 × 10^{3}, and it turns out that we can get a good enough approximation just by subtracting the digit term (that is, the number before the × in scientific notation) from 10 and using that as the value after the decimal point. It’s worth taking the time to familiarize yourself with this trick, because this is a highyield skill for MCAT math.
Using this trick, we can estimate the pKa of nitrous acid to be 3.6. If you do it with a calculator, you’ll find that the actual value is 3.4. This margin of error is close enough for the MCAT.
Estimating The pH
Now we need to tackle the acidbase ratio term. Before we do any math, though, let’s set expectations about the answer based on the passage information. Remember that the pK_{a} corresponds, by definition, to the pH where a weak acid is half protonated and half deprotonated (that is, where [A–] = [HA]). If we reduce the pH, the solution will become more acidic and HA will predominate. If we increase the pH, in contrast, the solution will become less acidic, and the deprotonated form (A–) will predominate, as shown in the diagram below.
Since the passage tells us that there’s a 4:1 acidbase ratio, or in plain English that there is 4 times as much of the acid as there is of its conjugate base, we can automatically conclude that the pH must be lower than the pK_{a}! At this point, we can eliminate any answer choices that are not lower than the pK_{a}.
However, the question may give us two answer choices that are lower than the pK_{a}, so we may have to determine how much lower the pH is. We can calculate this, but we should also use some general estimation techniques to minimize the math that we have to do. Recall that in the HendersonHasselbalch equation, we deal with the log of the ratio of [A–]/[HA]. This means that each increment of a power of 10 in the ratio will correspond to an increment of a single digit in the log of the ratio – so a 10x [A–]/[HA] ratio would correspond to a value of 1 for that term, a 100x [A–]/[HA] ratio would correspond to a value of 2, a 1000x [A–]/[HA] ratio would correspond to a power of 3, and so on. We’re told that the ratio is 4:1 in favor of the acid, so the [A–]/[HA] ratio is 1:4. This is less than a power of 10, so that means that we are looking for a pH that is lower than the pK_{a} by less than 1 – or, in other words, a pH between 2.6 and 3.6. There will almost certainly only be one answer choice that fits the bill.
Reflecting On The Problem
Let’s step back and summarize what we did here: (1) we recognized the equation we needed to use, (2) we used a shortcut to calculate the pK_{a}, (3) we used general reasoning about the scenario posed in the question to conclude that pH < pK_{a}, allowing us to eliminate answer choices, and finally (4) we used our knowledge of how logarithms work to estimate the pH range we’re looking for—all without any precise calculations!
It’s particularly worth noting that we could have used this problemsolving technique even if we forgot key details about the HendersonHasselbalch equation, like whether a + sign or a – sign comes after the pK_{a}, or whether it uses log[A–]/[HA] or log[HA]/[A–]. This is because we didn’t just memorize the equation – instead, we used our understanding of acidbase chemistry to make predictions.
Summing Up
In general, for MCAT chemistry, and for MCAT math in general, it’s a good idea to use shortcuts and estimations in your calculations and to be able to think through what a reasonable answer to the problem will be, for several reasons:
 To eliminate incorrect choices
 To ensure that you do the least work possible to get the right answer
 To serve as a reality check in case you make a silly mistake
Make sure you’re fully prepared for the MCAT exam. If you’re struggling with concepts like this or with other topics and sections, you should consider expanding your MCAT prep. Blueprint MCAT (formerly Next Step Test Prep) provides a Free MCAT Practice Bundle with plenty of resources to help you get started.
If you feel you need more help, we also provide guided prep options like our OneonOne Tutoring Programs and our comprehensive Online MCAT Course. Not sure what prep option is right for you? You can set up a free, no obligation consultation with one of our veteran Academic Managers. They can discuss your previous prep, your struggles, and your prep options. It can be a helpful conversation even if you don’t choose to work with us.
Good luck with your MCAT prep!
Written by Blueprint MCAT (formerly Next Step Test Prep) MCAT experts.
Search the Blog
Free Consultation
Interested in our Online MCAT Course or one of our OneonOne MCAT Tutoring packages? Set up a free consultation with one of our experienced Academic Managers!
Schedule NowPopular Posts

MCAT Blog How to Review MCAT FullLengths
Free MCAT Practice Account
Need great MCAT practice?Get the most representative MCAT practice possible when you sign up for our free MCAT Account, which includes a halflength diagnostic exam and one of our fulllength MCAT practice exams.
Learn More
Submit a Comment