Acetic acid's formula is CH3COOH, so it contains 4 hydrogen atoms, two carbon and two oxygen atoms.4 H2 C2 O
4.0 x 10-11
4.0 x 10-11
pH = 4 is about in the middle (4.7) of the values pH=pKa,1 and pH=pKa,2.This is an indication of H2PO4- abundantly being present, becauseat pH=2.14 it is halfway forming its conjugate acid H3PO4 andat pH=7.21 it is halfway forming its conjugate base HPO42-
4. The chemical equation is Cu + H2SO4 → CuSO4 + H2. Copper and sulfuric acid have the same coefficient (1), so the same number of moles of copper and sulfuric acid are used.
During an equilibrium in the following reaction.NH(3) + H(2)O NH(4)(+) + OH(-)NH(4) has the ability to give an H+ ion to OH ion and hence is the conjugate acid.
Acetic acid's formula is CH3COOH, so it contains 4 hydrogen atoms, two carbon and two oxygen atoms.4 H2 C2 O
To get the complex conjugate, change the sign in front of the imaginary part. Thus, the complex conjugate of -4 + 5i is -4 - 5i.
4.0 x 10-11
4.0 x 10-11
pH = 4 is about in the middle (4.7) of the values pH=pKa,1 and pH=pKa,2.This is an indication of H2PO4- abundantly being present, becauseat pH=2.14 it is halfway forming its conjugate acid H3PO4 andat pH=7.21 it is halfway forming its conjugate base HPO42-
4. The chemical equation is Cu + H2SO4 → CuSO4 + H2. Copper and sulfuric acid have the same coefficient (1), so the same number of moles of copper and sulfuric acid are used.
PO43- (phosphate) is the conjugate base of HPO42- (monohydrogen phosphate)
Yes, it does. The metal, Cobalt dissolves slowly in dilute sulphuric acid to form solutions containing the aqueous Co(II) ion together with hydrogen gas, H2. The equation is: Co (S) + H2So4 (aq) ---> Co^+2 (aq) + So4^-4 (aq) + H2 (g)
No
The formula for pure sulfuric acid is H2SO4 The mass of the components in g/mol is: H2 = 1 x 2 = 2 S = 32 O4 = 4 x 16 = 64 Total = 98
An acid (often represented by the generic formula HA [H+A−]) is traditionally considered any chemical compound that, when dissolved in water, gives a solution with a hydrogen ion activity greater than in pure water, i.e. a pH less than 7.0. That approximates the modern definition of Johannes Nicolaus Brønsted and Martin Lowry, who independently defined an acid as a compound which donates a hydrogen ion (H+) to another compound (called a base). Acids are described by a pKa which is essentially a hydrogen dissociation factor. Acids, discussed here in the general form HA, are proton (H+) donors and the pKa describes the dissociation behavior of that molecule. As a consequence, each acid exists in two species, the conjugate acid (HA) and the conjugate base (A-). When the pH is equal to the pKa of the molecule, the concentration of conjugate base is equal to that of conjugate acid and the molecule behaves in an acid/base equilibrium. A strong acid situation occurs when the molecule has completely dissociated to its conjugate base. As a consequence, every acid is considered a strong acid if the pH is 2 pH units higher or more than the pKa for the acid molecule. The 2 pH units is based on statistics. The best example is that of hydrochloric acid (HCl). The pKa of HCl is around -4. Since the pH scale is between 1 and 14, HCl completely dissociates regardless of the pH. For contrast, acetic acid has a pKa of about 4.76, and would act like a strong acid at pH's equal to or above 6.76, but would be a weak acid at all other pH's.