Acid chloric

Acid chloric
Acid chloric acid
Chloric acid
Tên khácChloric(V) acid
Nhận dạng
Số CAS7790-93-4
Ảnh Jmol-3Dảnh
SMILES
đầy đủ

  • O=Cl(=O)O

InChI
đầy đủ
  • 1/ClHO3/c2-1(3)4/h(H,2,3,4)
Thuộc tính
Công thức phân tửHClO3
Khối lượng mol84.45914 g mol−1
Bề ngoàiDung dịch không màu
Khối lượng riêng1 g/mL, solution (approxymate)
Điểm nóng chảy
Điểm sôi
Độ hòa tan trong nước>40 g/100 ml (20 °C)
Độ axit (pKa)ca. −1
Cấu trúc
Hình dạng phân tửpyramidal
Các nguy hiểm
Nguy hiểm chínhOxidant, Corrosive
Các hợp chất liên quan
Anion khácacid hydrobromic
acid hydroiodic
Cation khácAmoni chlorat
Natri chlorat
Kali chlorat
Hợp chất liên quanAcid hydrochloric
Acid hypochlorơ
Acid chlorơ
Acid pechloric
Trừ khi có ghi chú khác, dữ liệu được cung cấp cho các vật liệu trong trạng thái tiêu chuẩn của chúng (ở 25 °C [77 °F], 100 kPa).

Acid chloric có công thức là HClO3, là một acid có oxy của chlor. Là acid là một trong những acid mạnh (pKa ≈ −2.7), chỉ tồn tại ở dạng dung dịch. Acid chloric có tính oxy hóa mạnh; tác dụng với lưu huỳnh, phosphor, arsenic, khí lưu huỳnh dioxide. Giấy, bông bốc cháy ngay khi tiếp xúc với dung dịch HClO3 40%. Trong nước, nó mạnh tương đương với acid hydrochloric. Muối quan trọng nhất của nó là kali chlorat (KClO3). Acid chloric rất độc.

Tính chất

Axit cloric không ổn định về mặt nhiệt động theo hướng không cân đối.

Axit cloric ổn định trong dung dịch nước lạnh có nồng độ lên tới khoảng 30% và có thể điều chế các dung dịch có nồng độ lên tới 40% bằng cách làm bay hơi cẩn thận dưới áp suất giảm. Trên nồng độ này, dung dịch axit cloric bị phân hủy tạo ra nhiều loại sản phẩm, ví dụ:

8 HClO3 → 4 HClO4 + 2 H2O + 2 Cl2 + 3 O2

3 HClO3 → HClO4 + H2O + 2 ClO2

Tính chất hoá học

Acid chloric có thể phản ứng với nhiều kim loại trước dãy điện hoá của hydro:

2HClO3 + 2K → 2KClO3 + H2
2HClO3 + Ca → Ca(ClO3)2 + H2
6HClO3 + 2Al → 2Al(ClO3)3 + 3H2

Điều chế

Acid chloric có thể được điều chế bằng phản ứng giữa bari chlorat và acid sunfuric:

Ba(ClO3)2 + H2SO4 → 2HClO3 + BaSO4↓

Một phương pháp khác là đun nóng axit hypoclorơ, tạo ra axit cloric và hydro clorua:

3 HClO → HClO3 + 2 HCl

Nguy hiểm

Axit cloric là một tác nhân oxy hóa mạnh mẽ. Hầu hết các chất hữu cơ và chất dễ cháy sẽ bốc cháy khi tiếp xúc.

Tham khảo

  • Greenwood, Norman N.; Earnshaw, A. (1997), Chemistry of the Elements (ấn bản thứ 2), Oxford: Butterworth-Heinemann, ISBN 0-7506-3365-4
  • R. Bruce King biên tập (1994). “Chloric acid”. encyclopedia of Inorganic Chemistry. 2. Chichester: Wiley. tr. 658. ISBN 0-471-93620-0.

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