"You know what would make this poison really pop? A fistful of active charcoal and prompt medical treatment!"

enamel must be disciplined

Unrelated but they put out water at my work that's like just tap water sitting in a dispenser that they'll sometimes slice like, a couple oranges or lemons or cucumbers into. It adds no flavor and just wastes the fruit or cucumbers

What's the net pH after mixing a glass of alkaline water and a 'spritz of lemon'

I like it too. It's the best.

The most important thing to keep in mind with celebrity actors is that they make a living pretending to be someone/something they're not. And they're damn good at it too.

Not to cast doubt on everyone in that profession. Rather, proceed with an abundance of skepticism when considering celebrity endorsements.

Sorry to disappoint y’all. This is actually not so dumb. Chemically she makes a buffer solution.

How a Buffer Solution Works: Example with Baking Soda and Citric Acid

A buffer solution is a system that resists changes in pH when small amounts of acids or bases are added. Buffers are essential in chemistry and biology because many processes require a stable pH.

How Buffer Solutions Work

A buffer usually consists of a weak acid and its corresponding conjugate base (or a weak base and its conjugate acid). When an acidic or basic substance is introduced, the buffer reacts to neutralize the added ions, thus stabilizing the pH.

• When an acid (H⁺) is added, the buffer’s base component reacts with it, "soaking up" the excess H⁺ ions.
• When a base (OH⁻) is added, the acid part of the buffer reacts with it, neutralizing the excess OH⁻ ions.

The ability of a buffer to do this depends on the presence of both a weak acid and its conjugate base in appreciable amounts.

Buffer Example: Baking Soda (Sodium Bicarbonate) and Citric Acid

Ingredients Involved

• Baking soda (sodium bicarbonate, NaHCO₃): A weak base that can act as a proton acceptor.
• Citric acid (C₆H₈O₇): A weak acid, commonly found in citrus fruits.

When these two substances are dissolved in water, they interact according to the following reaction:

$$ \text{C}_6\text{H}_8\text{O}_7 + \text{NaHCO}_3 \rightarrow \text{C}_6\text{H}_7\text{O}_7^- + \text{Na}^+ + \text{H}_2\text{O} + \text{CO}_2\uparrow $$

This reaction creates a mixture containing both citric acid (weak acid) and its conjugate base (citrate ion).

How This Buffer System Functions

• If an acid is added to the solution (increasing H⁺), the citrate ion (Citrat-Anion) from the reaction will bind to the excess H⁺, lessening the pH shift.
• If a base is added (increasing OH⁻), the leftover citric acid will release H⁺, which neutralizes the OH⁻, keeping the pH stable.

Key Point:
This buffer is only effective within a certain pH range, which in this case is close to the pKa value of citric acid (around 3-7 depending on which proton is being lost, as citric acid is a triprotic acid).

Summary Table

This mixture resists pH changes thanks to the reversible interplay between the weak acid (citric acid) and its conjugate base (citrate ion), demonstrating the core principle of buffer solutions.