H2SO4 is more acidic if you have equal molar quantities and the same volume for each (ie. Concentration) as it's diprotic . so for example a solution containing 1moldm-3 of H2SO4 has a [H+]of 2moldm-3 whereas HCL and HNO3 have will have a [H+] of 1moldm-3. [H+] is the concentration of hydrogen ions in a solution and [h+] is a measure of acidity as [H+]=10-ph or rearranged Ph=-log[H+]
hydrochloric acid (HCl)Sulfuric acid (H2SO4)Nitric Acid (HNO3)
this is because when hcl and hno3 is mixed then it ionizes into h+and cl- and and and you may knaw rust is the mixing of foriegn particles in the pure substances. eg-fe+o2=fe2o3 so when gold is mixed with hcl and hnoc the it gives off aucl4. ie au pure gold is mixed with the pollutant cl4 similarly when h2so4 cant be used because s04 is not the neutral radical like no3 of hno3 thus s04 not being neutral and no3 being neutral h2so4 cant be used
The strong acids have pH=2 as HCl or H2SO4.
HNO3 is not used in redox titration because being a good oxidising ageant it oxidises the compound itself whereas HCL is a very volatile and it takes part in the reaction therefore H2SO4 is used in the reaction
Hydrofluoric acid (HF) Hydrochloric acid (HCl) and Nitric Acid (HNO3)
HCl H2SO4 HNO3
Some examples: HCl, HNO3, H2SO4.
HCl, HBr, HI, HNO3, H2SO4, HClO4
hydrochloric acid (HCl)Sulfuric acid (H2SO4)Nitric Acid (HNO3)
Some examples are: HNO3, HF, HCl, H2SO4.
An acid contain the cation hydrogen and an anion.Examples: HCl, HNO3, H2SO4 etc.
acids such as HCl, H2SO4 HNO3 etc
HCl H2SO4 HNO3 CH3COOH The common denominator is Hydrogen (H).
Acids contain hydrogen, such as HCl, HNO3, and H2SO4. MgCl is therefore not an acid.
SnO and SnO2 are soluble in HCl, HI, HNO3, H2SO4, etc.
Any Arrhenius acid as HCl,HNO3, H2SO4 etc.
Monoprotic: HCl, CH3COOH (acetic acid)Diprotic: H2SO4, HOOCCOOH (oxalic acid)Triprotic: H3PO4, C3H4OH(COOH)3(citric acid)(All acidic protons are bold)