Conjugate pairs and pH · 共轭对和 pH
| English | 中文 | Pinyin · 拼音 |
|---|---|---|
| conjugate base/ˈkɒndʒuːɡeɪt beɪs/ | 共轭碱 | gòng è jiǎn |
| conjugate acid/ˈkɒndʒuːɡeɪt ˈæsɪd/ | 共轭酸 | gòng è suān |
| weak acid/wiːk ˈæsɪd/ | 弱酸 | ruò suān |
| strong acid/strɒŋ ˈæsɪd/ | 强酸 | qiáng suān |
| strong alkali/strɒŋ ˈælkəlaɪ/ | 强碱 | qiáng jiǎn |
Acids, bases and their partners
- When an acid loses $\text{H}^+$, what's left is its conjugate base 共轭碱.
- pH and the equilibrium constants put numbers on acidity.
- The method to find pH depends on the acid or base.
酸、碱和它们的伙伴
- 当一个酸失去 $\text{H}^+$ 时,剩下的是它的共轭碱(conjugate base)。
- pH 和平衡常数给酸性定上数。
- 找 pH 的方法取决于酸或碱。
The conjugate base of CH₃COOH is: · CH₃COOH 的共轭碱是:
Removing one H⁺ from the acid leaves its conjugate base; the two differ by a single proton. · 从酸移除一个 H⁺ 留下它的共轭碱;这两个相差一个质子。
An acid and the base formed when it loses a proton are a conjugate . · 一个酸和它失去一个质子时形成的碱是一个共轭。
e.g. HA and A⁻. · 例如 HA 和 A⁻。
Conjugate acid 共轭酸–base pairs
- An acid loses $\text{H}^+$ → its conjugate base; a base gains $\text{H}^+$ → its conjugate acid.
- The two differ by one $\text{H}^+$ — a conjugate pair. E.g. $\text{CH}_3\text{COOH}$ / $\text{CH}_3\text{COO}^-$.
Conjugate acid-base pairs differ by one proton
共轭酸碱对
- 一个酸失去 $\text{H}^+$ → 它的共轭碱;一个碱得到 $\text{H}^+$ → 它的共轭酸(conjugate acid)。
- 这两个相差一个 $\text{H}^+$——一个共轭对(conjugate pair)。例如 $\text{CH}_3\text{COOH}$ / $\text{CH}_3\text{COO}^-$。
共轭酸碱对相差一个质子
pH and H⁺ concentration · pH 与 H⁺ 浓度
pH = −log[H⁺]: slide it and watch [H⁺] change tenfold per unit. A conjugate acid–base pair differ by a single proton. · pH = −log[H⁺]:滑动它,看 [H⁺] 每变化一个单位就改变十倍。一对共轭酸碱只相差一个质子。
pH is defined as: · pH 定义为:
pH = −log[H⁺]; so [H⁺] = 10^(−pH). · pH = −log[H⁺];所以 [H⁺] = 10^(−pH)。
A larger Ka (smaller pKa) means the acid is: · 一个更大的 Ka(更小的 pKa)意味着酸是:
A bigger acid dissociation constant means more dissociation, so a stronger acid. · 一个更大的酸解离常数意味着更多解离,所以一个更强的酸。
Match each acid-base term. · 匹配每个酸碱术语。
Each item links the term to its correct meaning. · 每一项把术语链接到它正确的含义。
pH and the constants
- $\text{pH} = -\log[\text{H}^+]$, so $[\text{H}^+] = 10^{-\text{pH}}$.
- weak acid 弱酸: $K_a = \dfrac{[\text{H}^+][\text{A}^-]}{[\text{HA}]}$, and $\text{p}K_a = -\log K_a$ (larger $K_a$ = stronger acid).
- water: $K_w = [\text{H}^+][\text{OH}^-] = 1.0 \times 10^{-14}$ at 298 K.
The pH scale: pH =-log of the hydrogen-ion concentration
pH 和常数
- $\text{pH} = -\log[\text{H}^+]$,所以 $[\text{H}^+] = 10^{-\text{pH}}$。
- 弱酸:$K_a = \dfrac{[\text{H}^+][\text{A}^-]}{[\text{HA}]}$,而 $\text{p}K_a = -\log K_a$(更大的 $K_a$ = 更强的酸)。
- 水:$K_w = [\text{H}^+][\text{OH}^-] = 1.0 \times 10^{-14}$ 在 298 K。
To find [H⁺] for a weak acid, you use: · 要找一个弱酸的 [H⁺],你用:
A weak acid is only partly ionised, so [H⁺] = √(Ka × [HA]); a strong acid uses [H⁺] = concentration. · 一个弱酸只部分电离,所以 [H⁺] = √(Ka × [HA]);一个强酸用 [H⁺] = 浓度。
Calculating pH
- strong acid 强酸 (fully ionised): $[\text{H}^+]$ = acid concentration, then $-\log$.
- strong alkali 强碱: find $[\text{OH}^-]$, then $[\text{H}^+] = K_w / [\text{OH}^-]$.
- weak acid: $[\text{H}^+] = \sqrt{K_a \times [\text{HA}]}$.
计算 pH
- 强酸(完全电离):$[\text{H}^+]$ = 酸浓度,然后 $-\log$。
- 强碱:找 $[\text{OH}^-]$,然后 $[\text{H}^+] = K_w / [\text{OH}^-]$。
- 弱酸:$[\text{H}^+] = \sqrt{K_a \times [\text{HA}]}$。
You've got it
- conjugate pair = acid and base differing by one $\text{H}^+$
- $\text{pH} = -\log[\text{H}^+]$; $K_a$ (bigger = stronger acid); $K_w = 1.0 \times 10^{-14}$
- strong acid: $[\text{H}^+]$ = conc; strong alkali: via $K_w$; weak acid: $\sqrt{K_a[\text{HA}]}$
你掌握了
- 共轭对 = 相差一个 $\text{H}^+$ 的酸和碱
- $\text{pH} = -\log[\text{H}^+]$;$K_a$(更大 = 更强的酸);$K_w = 1.0 \times 10^{-14}$
- 强酸:$[\text{H}^+]$ = 浓度;强碱:经 $K_w$;弱酸:$\sqrt{K_a[\text{HA}]}$