A solution containing 45.00 ml of 0.0500 M metal ion buffered to pH = 10.00 was...

A solution containing 45.00 ml of 0.0500 M metal ion buffered to pH = 10.00 was titrated with 0.0400 M EDTA. Answer the following questions and enter your results with numerical value only.

Calculate the equivalence volume, V_e, in milliliters.

Calculate the concentration (M) of free metal ion at V = 1/2 V_e.

Calculate the fraction (α_Y^4-) of free EDTA in the form Y^4-. Keep 2 significant figures.

If the formation constant (K_f) is 10^12.00. Calculate the value of the conditional formation constant K_f’ (=α_Y^4- * K_f) and enter your result as scientific notation form.

Calculate the concentration (M) of free metal ion M⁺ at V = V_e. (Use the K_f' calculated above)

Expert Solution

queen_honey_blossom answered 2 years ago

A solution containing 10.00 mL of 0.0500 M metal ion buffered to pH = 10.00 was...

A solution containing 10.00 mL of 0.0500 M metal ion buffered to pH = 10.00 was titrated with 0.0400 M EDTA. Calculate the fraction (αY4-) of free EDTA in the form Y4−. Keep 2 significant figures.

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A solution containing 45.00 mL of 0.0500 M metal ion buffered to pH = 11.00 was titrated with 0.0400 M EDTA. Answer the following questions and enter your results with numerical value only. Calculate the equivalence volume, Ve, in milliliters. 56.2 You are correct. Your receipt no. is 157-1182 Help: Receipt Previous Tries Calculate the concentration (M) of free metal ion at V = 1/2 Ve. 0.0154 You are correct. Your receipt no. is 157-4788 Help: Receipt Previous Tries Calculate...

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A solution containing 40.00 mL of 0.0500 M metal ion buffered to pH = 12.00 was titrated with 0.0400 M EDTA. Calculate the fraction (αY4-) of free EDTA in the form Y4−. Keep 2 significant figures.

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