Discussion Overview
The discussion revolves around calculating the pH of a solution formed by mixing 50 ml of 0.004M H2CrO4 with 50 ml of 0.005M HNO3. Participants explore the roles of these substances as acids, the need for dissociation constants, and the implications of strong versus weak acids in the calculation.
Discussion Character
- Homework-related
- Debate/contested
- Mathematical reasoning
Main Points Raised
- One participant initially identifies H2CrO4 as the acid and HNO3 as the base, questioning the approach taken.
- Another participant corrects this by stating that both substances are acids, prompting a discussion about their dissociation.
- It is noted that HNO3 is a strong acid and dissociates completely, while H2CrO4 is not a strong acid, requiring consideration of its dissociation constant (Ka).
- A calculation is presented for the concentration of H+ ions from HNO3, leading to a proposed pH value, but this is met with skepticism and corrections from other participants.
- One participant suggests looking up the Ka for H2CrO4 and setting up an equilibrium equation as a necessary step in the calculation.
Areas of Agreement / Disagreement
There is disagreement regarding the classification of the substances involved and the correct approach to calculating pH. Some participants assert that H2CrO4 requires Ka for accurate calculations, while others challenge the calculations presented without reaching a consensus.
Contextual Notes
Participants express uncertainty about the dissociation of H2CrO4 and the implications of using Ka in the calculations. There are unresolved mathematical steps and differing interpretations of the acids' behavior in solution.
Who May Find This Useful
Students working on acid-base chemistry, particularly those dealing with pH calculations involving strong and weak acids.
