What volume (mL) of 0.025 M HNO3 is necessary to titrate 5.2 mL of 0.046 M Ca(OH), solution to the endpoint? Please give the answer to 1 decimal place.
Q: What volume (in mL) of 0.2300 M HBr is required to neutralize 50.00 mL of 0.7000M KOH?
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Q: What volume (in mL) of 0.2800 M HBr is required to neutralize 50.00 mL of 0.7000M KOH?
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Q: What volume (in mL) of 0.2600 M HBr is required to neutralize 50.00 mL of 0.7000 M KOH?
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Q: What volume (in mL) of 0.2850 M HBr is required to neutralize 50.00 mL of 0.7000 M KOH?
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Q: You titrate a 450 mL HNO3 solution with 0.40 M NaOH. If it takes 75 mL of NaOH to reach the…
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Q: What volume (in mL) of 0.2300 M HBr is required to neutralize 50.00 mL of 0.7000 M KOH?
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- Sketch a pH curve for the titration of a weak acid (HA) with a strong base (NaOH). List the major species, and explain how you would go about calculating the pH of the solution at various points, including the halfway point and the equivalence point.Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
- Consider a 10.0% (by mass) solution of hypochlorous acid. Assume the density of the solution to be 1.00 g/mL. A 30.0-mL sample of the solution is titrated with 0.419 M KOH. Calculate the pH of the solution (a) before titration. (b) halfway to the equivalence point. (c) at the equivalence point.A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.5. A 25.00-mL portion of a H₂SO4 solution was titrated with a 0.256 M KOH solution. To reach the equivalence point required 31.2 mL of the base. a) Write a chemical equation for the titration. (pai) sling (usindost to ofgez low bocistdo 028 and daw ba b) What was the molarity of the sulfuric acid solution? ods anw red 02),A 1,004 v 20.20 alde tximo Tol ment bonisado od vlasnoor (ans: 0.160 M)
- 3. Cal culate Nattz POy:(Ka, kaz and tas of HsPO4 6.32x10-8 and 4.5x10-13 he ott of a o.0400M Shutin of ane 7.11 メL65 respectively). 4. Con Sider the titration of 1w.00ml of a 0.200M Solution of he hypothetical acid tzA uith o.loc Soclium hydroxide. Enourhg hat Kay = (. 00 k1o-8, and kag = 1.00 xLo 12 Calculate ka after he addition of a) 1o. oml Na OH =l:00x16", E1:00x104 9 20.oml Na OH ) 30. omL Na ott d) 40.0ml Na OHConsider the following infermation about sulfurous acid, a diprotic acid (11,S0,L LSO3=HSO, +1I* pK=1.81 HSO, S0,+H pK2-691 The titration curve for sodism sulfite, Na SO, with standard HCl is shown below PH VI V2 ml, HO added What are the major species present al point 3? O NoCalculate the pH during the titration of 20.00 mL of 0.1000 M KOH with 0.2000M HBr solution after the following additions of acid (show work): a) O mL b) 5.000 mL c) 10.00 mL d) 15.00 mL
- Qy A 50ml 0.1IM CeH:COOH( K= 10-)is diluted to 100 m! and titrated with 0.2 M KOH 1- Find the PH before any base is added 2- Find the PH when 15 ml of base has been added. 3. Find the PH at the equivalence point 4. Find the PH when 30 ml of base has been added 5- Draw the approximate titration curve, and discuss the feasibility of the titration.Q1) A sada- Lime Sample is 90% NaoH and 10% CaO• If 3gm is dissolved in 250 ml, what is the tutal normadity of the Selution as abase ? How many milliliters of O.57N H2 S@4 would be requiredd to titrate i00 me of the Solution ? Ans.s ( 0.309 N, 60.59 ml) Q12) How much water that required add to 200 ml HNO, ( densly = 1.285 gm/ml) Contains 46 wt% acid to Convert lo wt% acid solution? Ars. : 919.6 ml12. Collect a sample of lake water; a) 100 mL titrate with 0.05N HCI to HCO3 eq.pt. and we need to add 0.5 mL of acid solution. What is the CO3 ALK as M and mg CaCO3/L? b) 100 mL titrate with 0.03N NaOH to CO; eq.pt. and we need to add 0.6 mL of base solution. What is the OH ALK as M and mg CaCO3/L? c) What is the Cr and pH value?