ANSWER ASAP PLEASE The Ca2+ in a 25.00mL of underground powder was titrated with 28.60 mL of 0.01350 M EDTA. Calculate the concentration of Ca2+ in ppm. Round off your final answer to four significant figures.
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ANSWER ASAP PLEASE
The Ca2+ in a 25.00mL of underground powder was titrated with 28.60 mL of 0.01350 M EDTA. Calculate the concentration of Ca2+ in ppm. Round off your final answer to four significant figures.
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- What is the maximum metallic concentration in 100.0 liters of water from a metallic hydroxide with a Ksp = 3.99 x 10-20 at pH 3.0, 7.0, and 10.0? Show all work and report final answers with three significant figures.Calculate the volume of 0.0500 M EDTA needed to titrate 29.13 mL of 0.0598 M Mg(NO3 )2. Use a MW value in 4 decimal places.A water sample is approximated to have a total hardness equal to 120.0ppm. How many milliliters of 0.01000N EDTA will be needed to titrate 250.00mL of the said water sample?(MM CaCO3=100.09g/mol). ** Need asap pls. Thanks.
- mix 500 ml of 0.1 M HCl solution with 300 ml of 2 M Ba (OH) 2 solution a) indicate the environment of the solution after mixing b) What color will the detectors, phenophthalein and litmus get?Procedure Preparation of Dilute Solution of Vinegar • Using a 10 mL pipette, transfer 10mL of vinegar into 100 mL volumetric flask. • Dilute to mark of the volumetric flask using distilled water. B. Titration of Diluted Solution of Vinegar • Transfer 25 mL of diluted solution to 250 mL Erlenmeyer flask. • Add 0.5 mL phenolphthalein indicator. Set aside. • Transfer 50mL of 0.110 M NaOH into a 50 mL burette. • Titrate the diluted solution until the phenolphthalein endpoint (very faint pink). • Record volume of NaOH used. Answer the question: What is the experimentally determined concentration of acetic acid in your vinegar solution: (Please give your answer to three significant figures.) ______ M Acetic AcidA 25.00 mL unknown water sample is titrated with a standardized 0.0140 M EDTA solution. It is determined that 8.54 mL of EDTA is required to reach the end point. The blank titre was determined to be 1.50 mL. Determine the concentration of Calcium in the water sample in ppm. (mwt. of CaCO3 = 100.0892 g/mol).
- An unknown sample of Cu2+gave an absorbance of 0.262. Then 1.00 mL of solution containing 100 ppm (ug/mL)Cu2+was mixed with 95.0 mL of the unknown and the mixture was diluted to 100 mL in a volumetric flask with deionized water. The absorbanceof the new solution was 0.500. a.Denoting the initial unknown concentrationas [Cu2+]i,write an expression for the final concentrationafter dilution [Cu2+] b.Find [Cu2+]in the unknown.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) 25.00 ml water sample, 19.040 ml of 4.965x 10−3 M EDTA solution to reach the endpoint.A 15.00 g sample containing mixed alkali and other inert components was dissolved and diluted to 300 mL with water. A 20 mL aliquot was titrated with 5.02 mL of 0.5352 M HCl to reach PHP endpoint. Another 20 mL aliquot was titrated to the BCG endpoint, using up 18.87 mL of titrant in the process. Note: Answer in two decimal places only. If there is no answer, type in 0.00. Use the molar masses 105.989 ?/??l ??2cO3 and 84.007 g/mol NaHCO3 indicated. The volume of titrant needed to neutralize NaOH is _________ mL.The volume of titrant needed to neutralize Na2CO3 is _____________ mL.The volume of titrant needed to neutralize NaHCO3 is _____________ mL. The mass of NaOH is ___________ g.The mass of Na2CO3 is __________ g.The mass of NaHCO3 is __________ g. The percent weight of NaOH is __________ %.The percent weight of Na2CO3 is __________ %.The percent weight of NaHCO3 is __________ %.
- A 50.00-mL aliquot of solution containing 0.310 of MgSO4 (FM 120.37) in 0.500 L required 37.77 mL of EDTA solution for titration. How many milligrams of CaCO3 (FM 100.09) will react with 1.00 mL of this EDTA solution? Answer in 3 significant figures. Do not include the unit. need asapNeed solution to all parts if not answered I'll downvote solution Find the pH during the titration of 20.00 mL of 0.1910 M benzoic acid, C6H5COOH (Ka = 6.3 10-5), with 0.1910 M NaOH solution after the following additions of titrant. (a) 0 mL (b) 10.00 mL (c) 15.00 mL (d) 20.00 mL (e) 25.00 mLFind the pCl in a 20 mL of a 0.10 M Cl- solution after addition of 0, 10, 20, and 30 mL of 0.10 M AgNO3 . Ksp = 1.0x10-10