Find the conditional formation constant for Ca(EDTA)2- at pH 11.00, where log Kf is 10.65 and aya- is 0.81. K = Find the concentration of free Ca?+ in 0.030 M Na,[Ca(EDTA)] at pH 11.00. [Ca?+] = M
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![Find the conditional formation constant for Ca(EDTA)²- at pH 11.00, where log K is 10.65 and aya- is 0.81.
K =
Find the concentration of free Ca?+ in 0.030 M Na,[Ca(EDTA)] at pH 11.00.
[Ca?+] =
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fecf65368-5b58-4f50-aa93-38dd34561753%2Fa8b21ef4-3bdb-403f-8152-ad4c6685cdd8%2F5itdm6c_processed.jpeg&w=3840&q=75)
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- Construct a titration curve that is expected to be obtained by titration 50.00mL of 0.1000M Sr2+ with 0.1000M EDTA at pH 11. Kf = 4.3 x 10^8. Use the following volumes to construct the curve: 0.00, 10.00, 30.00, 40.00, 45.00, 50.0, 55.00, 60.00 and 70.00mL.A deepwell water sample of 100 mL was titrated with 0.010 M EDTA at pH 10 ( with Mg-EDTA pH 10 buffer reagent) and consumed 31 mL. Calculate the Total Hardness of the water sample as mg CaCO3. Ans in 3 sig figures. no need to write the unit.A deepwell water sample of 100 mL was titrated with 0.010 M EDTA at pH 12 and consumed 31 mL. Calculate the Calcium content of the water sample in mg/L.
- In the titration of 25.00 mL of a water sample, it took 20.840 mL of 4.350x 10−3 M EDTA solution to reach the endpoint. Calculate the number of moles of EDTA required to titrate the water sample. (enter your answer with 3 significant figures) 9.07×10-5 The total hardness is due to one or a combination of Ca2+, Mg2+, and Fe2+ in your sample. It is convenient to express this hardness as though it was entirely due to Ca2+. Making this assumption, determine the number of moles of Ca2+ present in the bottled water sample titrated. (enter your answer with 3 significant figures) he total hardness is always listed in parts-per-million (ppm) of CaCO3 (or mg CaCO3 / Kg H2O). Since the density of water is 1.0 g/mL, one ppm would be the same as the number of mg of CaCO3 per liter of water. Determine the number of moles of CaCO3 present in the titrated sample of water, assuming that all the Ca2+ combines with CO32−. (enter your answer with 3 significant figures)“This EDTA solution was used to titrate a 100 ml sample of water, adjusted to pH 10, using EBT as the indicator. The titration required 11.23 ml to reach a blue endpoint. Calculate the total concentration of Ca^2+ and Mg^2+ in the water. (The EDTA reacts i a 1:1 mole ratio with both Ca^2+ and Mg^2+.) Express the concentration in moles of metallic cation per liter.” I have found the molarity from part a.) to be 9.9788 x 10^-3. How do I solve part b?The formation constant (Kf) for calcium reacting with EDTA is 6.2 x108. A calcium-EDTA titration was done at a pH = 10.00, where the fraction of species of Y4- is approximately 0.39, what would be the value for the conditional formation constant (Kf') for the reaction? Group of answer choices 6.2 x 108 2.4 x 108 4.5 x 1011 1.0 x 1010
- A deepwell water sample of 100 mL was titrated with 0.010 M EDTA at pH 12 and consumed 31 mL. Calculate the Calcium content of the water sample in mg/L. Ans in 3 sig figures. no need to write the unit.In a titration, the following masses were recorded from an unknown substance that contain some amount of KHP in three experimental solutions 0.44, 0.437, and 0.437, if the volume of NaOH IN THE exp are 5, 10, and 8 respectively in order to the masses of unknown substances.1. Find the mass of KHP of each experiment 2.Find % KHP 3. Find average % KHP 4.find standard deviation.( Note; in a previous three 100% KHP experiments the average molarity of NaOH in each experiment are shown below average molarity=5.30x 10^-4+ 4.137x10^-4 + 5.0x10^-4 divided by 3 = 4.81x10^-4 ).Calculate the silver ion concentration after the addition of 5.00, 30.00, 40.00, 45.00 and 50.00 ml of 0.05000 M AgNO3 to 50.0 mL of 0.0400 M KBr. Construct a titration curve from these data plotting pAg as a function of titrant volume (Ksp (AgBr)=5.0 x 10-13 )
