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Iodous acid (HIO,) is a weak acid that dissociates in water as follows. HIO,(aq) + H,0(1) ==H;0*(aq) + 10, (aq) The acid-dissociation constant (K.) for iodous acid is 3.2x10-5. Calculate the percent ionization (percent dissociation) if the initial concentration of iodous acid was 0.35 M. Step 1 of 5 Recall the relationship between an acid's dissociation constant (K) and its percent ionization (percent dissociation). [H,0*lequilibrium x 100% [HA]initial % ionization of an acid = In this equation, [HA]initial is the initial concentration of the acid in molarity and [H,0*]equilibrium is the concentration of H,0+ ions at equilibrium in molarity. Before calculating the percent ionization, the K, of iodous acid must be used to find the following. O [H,0*linitial O [HAJequilibrium O [HAJinitial [H,0*]equilibrium Step 2 of 5 Write the acid dissociation constant expression for this given reaction. HIO (2a) t H O O = H ot(aa) 1 TO -( ag)

Iodous acid (HIO,) is a weak acid that dissociates in water as follows. HIO,(aq) + H,0(1) ==H;0*(aq) + 10, (aq) The acid-dissociation constant (K.) for iodous acid is 3.2x10-5. Calculate the percent ionization (percent dissociation) if the initial concentration of iodous acid was 0.35 M. Step 1 of 5 Recall the relationship between an acid's dissociation constant (K) and its percent ionization (percent dissociation). [H,0*lequilibrium x 100% [HA]initial % ionization of an acid = In this equation, [HA]initial is the initial concentration of the acid in molarity and [H,0*]equilibrium is the concentration of H,0+ ions at equilibrium in molarity. Before calculating the percent ionization, the K, of iodous acid must be used to find the following. O [H,0*linitial O [HAJequilibrium O [HAJinitial [H,0*]equilibrium Step 2 of 5 Write the acid dissociation constant expression for this given reaction. HIO (2a) t H O O = H ot(aa) 1 TO -( ag)

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Iodous acid (HIO,) is a weak acid that dissociates in water as follows. HIO,(aq) + H,0(1)=H;0*(aq) + I02 (aq) The acid-dissociation constant (K) for iodous acid is 3.2x10-5. Calculate the percent ionization (percent dissociation) if the initial concentration of iodous acid was 0.35 M. Step 1 of 5 Recall the relationship between an acid's dissociation constant (K) and its percent ionization (percent dissociation). [H,0*1e equilibrium x 100% % ionization of an acid = [HA]initial In this equation, [HA]nitial is the initial concentration of the acid in molarity and [H,0*]equilibrium is the concentration of H,0+ ions at equilibrium in molarity. Before calculating the percent ionization, the K, of iodous acid must be used to find the following. O [H,0*]initial O [HAJequilibrium [HA]initial [H,0*]equilibrium Step 2 of 5 Write the acid dissociation constant expression for this given reaction. HIO,(aq) + H,0(1) =H,0*(aq) + I0, (aq) The acid dissociation constant expression for the reaction of HIO, with water is the following. (Concentration equilibrium expressions take the general form: K. = [C]° / [A]ª . [B]°. Subscripts and superscripts that include letters must be enclosed in braces {}.) chemPad Help Greek - H20 H_20 Your answer differs too much from the expected answer to provide useful feedback. Note that the concentrations expressed in the acid dissociation constant are equilibrium concentrations, which must be determined. Write the expression for the acid-dissociation or base-dissociation constant for a specified weak acid or base.
Transcribed Image Text:Iodous acid (HIO,) is a weak acid that dissociates in water as follows. HIO,(aq) + H,0(1)=H;0*(aq) + I02 (aq) The acid-dissociation constant (K) for iodous acid is 3.2x10-5. Calculate the percent ionization (percent dissociation) if the initial concentration of iodous acid was 0.35 M. Step 1 of 5 Recall the relationship between an acid's dissociation constant (K) and its percent ionization (percent dissociation). [H,0*1e equilibrium x 100% % ionization of an acid = [HA]initial In this equation, [HA]nitial is the initial concentration of the acid in molarity and [H,0*]equilibrium is the concentration of H,0+ ions at equilibrium in molarity. Before calculating the percent ionization, the K, of iodous acid must be used to find the following. O [H,0*]initial O [HAJequilibrium [HA]initial [H,0*]equilibrium Step 2 of 5 Write the acid dissociation constant expression for this given reaction. HIO,(aq) + H,0(1) =H,0*(aq) + I0, (aq) The acid dissociation constant expression for the reaction of HIO, with water is the following. (Concentration equilibrium expressions take the general form: K. = [C]° / [A]ª . [B]°. Subscripts and superscripts that include letters must be enclosed in braces {}.) chemPad Help Greek - H20 H_20 Your answer differs too much from the expected answer to provide useful feedback. Note that the concentrations expressed in the acid dissociation constant are equilibrium concentrations, which must be determined. Write the expression for the acid-dissociation or base-dissociation constant for a specified weak acid or base.
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