If 0.2997 g of potassium iodate (KIO3) are dissolved in 25.00 mL of distilled water, what is the resulting molarity (M)? Give a brief explanation about why this is a very precise concentration to use. In other words, what makes potassium iodate such a good reagent with which to work in lab?
firstly, we calculate the molarity of potassium iodate.
since , Molarity = no. Of mole/ volume (in Litre)
So, number of moles of potassium iodate= weight in g / molar mass.
= 0.2997/214 = 0.0014
And volume = 25 ml/1000l = 0.025 Litre.
Therefore, Molarity M= 0.0014/0.025 = 0.056 mol/litre.
Now, Why makes potassium iodate such a good reagent ??
the answer is -
Since potassium iodate is a salt of iodine , and it is quite stable reagent.it has much higher shelf life. It can be stored in lab and can be used for a long time.
As well, potassium iodate is a thyroid blocking agent and also it can be used as a maturing agent in baking sometimes.
These unique properties makes potassium iodate a good reagent with which to work in lab.
please upvote
If 0.2997 g of potassium iodate (KIO3) are dissolved in 25.00 mL of distilled water, what...
0.6573 g of potassium iodate is dissolved and diluted to a volume of 100.0 mL. Then 25.00 mL of this stock solution is pipetted into a 100.0 mL volumetric flask which is filled to the mark with water. What is the concentration of the final standard solution in mol/L? Include units in your answer, and round the final answer to the correct number of significant figures.
A 0.1358-g portion of potassium iodate (MW 214.00), about 2 g of potassium iodide, and 2 mL of 6 M hydrochloric acid were dissolved in 25 mL of distilled water. The triiodide formed during the ensuring reaction was titrated to the starch endpoint with 31.94 mL of a thiosulfate solution. A 25.00-mL triiodide sample solution was titrated to the endpoint with 21.33 mL of the standardized thiosulfate solution. Calculate the concentrations of the thiosulfate solution and the triiodide solution.
25.00 g of potassium hydrogen phosphate (K HPO4) is dissolved in enough water to make 125.0 mL of a solution with a density of 1.22 g/mL. What is the concentration of the solution in % (m/m). % (m/v). molarity, mosM and mEq/L of the potassium ion? Note: K2HPO4 has a molar mass of 174.2g/mole. What would be the final molarity of the above solution if you were to dilute it by adding 175 mL of water?
Exactly 0.5458 g of potassium chloride was placed in a 200 mL volumetric flask (class A). It was dissolved and diluted with distilled water up to the 200-mL mark. Calculate: (a) concentration of KCl in the resulting solution in g/L (b) concentration of potassium K in this solution in g/L (c) molarity of this solution
7.920 g of potassium oxalate is dissolved in water to make 450.0 mL of solution. What is the molarity of the potassium oxalate solution ?
15 g of potassium chlorate are dissolved in water to produce 250 mL of solution. What is the solution's molarity?
A 0.350-g sample pf an acid, HX, is dissolved in 25.00 mL of water. The resulting solution is titrated with 0.140 M NaOH solution, and 25.40 mL of the base solution is required to neutralize the acid. Calculate the molar mass of the acid.
6: Suppose 50.0 g of pure potassium hydroxide is dissolved in 250.00 mL water ( Solvent: -0.9987 g/mL). Given the density of the solution is 1.020 g/mL, what will be the molarity of the solution. (Hint: You need to find the volume of the solution)
how do I calculate the isolated moles and molarity of the 0.2M KIO3? 0.1 M Sulfuric Distilled Solution A Mixturel Mixture II Mixture III Mixture IV 0.20 M KIO3 Solution 5 mL 5 mL 10 mL 10 mL Acid 0 mL 0.5 mL 0 mL 0.5 mL water 15 ml 14.5mL 10 mL 9.5 mL Lalculations: I. (6pt) Calculate the total number of moles of iodate ion present in each 0.2 M KlO3 solution. Calculate the molarity of iodate ion...
A 1.04 g sample of KBr is dissolved in water to give 155 mL of solution. This solution is then added to 165 mL of 0.015 M aqueous Pb(NO3)2, in an attempt to remove the toxic lead(II) ions from the solution via precipitation as insoluble PbBr2(s). The precipitation reaction that occurs is: Pb2+ (aq) + 2 Br (aq) ---> PbBr2 (s) At the end of the reaction, what is the concentration (in molarity) of nitrate ions in the solution? Note:...