1. Calculate the pH of the solution with hydrogen concentration provided below: a. [H*] = 1.0 x 10² b. [H*] = 2.0 x 104 c. [H*]= 3.0 x 10s d. [H*]= 1.0x 10°8 e. [H*]= 2.50 x 104 f. [OH']= 1.11 x 104
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- 1. Calculate the pH of the following solutions: A. [H+] = 1.36 x 10-9 M В. [ОН] —D 3.86 x 10-8 М 2. Calculate the pOH of the following solutions: A. [OH-] = 8.6 x 10-8 M В. рH %3D 3.2 3. What is the pH of a buffer prepared by mixing 100 ml 0.050 mM NAH2PO4 and 25 ml 0.075 mM Na2HPO4? (рКa1%32.2; рКо23 7.21; pКаз312.7)Calculate the concentration of Y4-ion in 0.0100 M EDTA solution at pH 6. α4 = 2.2 x 10-5 for pH 6.Calculate the pH of the resulting solution if 23.0 mL of 0.230 M HCl(aq) is added to 33.0 mL of 0.230 M NaOH(aq). pH = Calculate the pH of the resulting solution if 23.0 mL of 0.230 M HCl(aq) is added to 13.0 mL of 0.330 M NaOH(aq). pH=
- What is the approximate pH of a solution labeled 6 x 10-5 M HBr? * 4.2 4.5 5.8 9.8 8.2Calculate the ratio [CH3COOH]/[N2CH3COO] that gives a solution with pH = 5.00? * 0.28 0.36 0.44 0.56 0.63If an aqueous solution has a hydroxyl ion concentration of 1 × 10-6 M, what is the concentration of hydrogen ion ([H+]) ? [H+] = 1.0 x10-5 M
- Estimate the pH of a 7.18 x 106 M HF solution. You can calculate the lowest possible pH, knowing that the actual value will be higher. Your answer should contain 3 decimal places as this corresponds to 3 significant figures when dealing with logs. pH will be above Select the solution with the highest pH. Multiple Choice 0.0225 MLIOH 0.0225 MH2CO3 0.0225 MCH3NH2Calculate the theoretical pH of a Tris buffer (pH 8.0) at 0 ºC. Assume that room temperature is 22 ºCCalculate the normality of a solution that contains 4.5 g of (COOH)2 in 3000 mL of solution? (Assume the (COOH)2 is to be completely neutralized in an acid-base * reaction.) 0.033 N O 0.33 N O 0.166 N O 0.0166 N 0.45 N O 0.045 N 000.0 OO
- You need to prepare an acetate buffer of pH 5.43 from a 0.621 M acetic acid solution and a 2.95 M KOH solution. If you have 730 mL of the acetic acid solution, how many milliliters of the KOH solution do you need to add to make a buffer of pH 5.43? The pKa of acetic acid is 4.76. Be sure to use appropriate significant figures.A solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. A. Can the metal ions be separated by slowly adding Na2CO3 aq solution? Assume that for successful separation 99% of the metal ion must be precipitated before the other metal ion begins to precipitate, and assume no volume change on addition of Na2CO3 solution. Ksp of CuCO3 = 1.4 x10-10 Ksp of NiCO3 = 1.42X 10-7 B. If you need to redissolve the salt that was first precipitated, what pH will you use and why ? Write your answers in template provided. Upload your step by step solution for A.1) Calculate the required gram of Tris-Hcl to prepare 1M, 100 ml Tris-HCl (Tris Stock) with mol and Molarity formula. 2)Calculate the required gram of EDTA to prepare O.5M, 100 ml EDTA (EDTA stock) mol and Molarity formula. 3.) Calculate the required volume of Tris Stock to prepare buffer A which contains 25 mM Tris-Hcl with final volume is 100 ml by using M1V1 =M2V2 formula 4) Calculate the required volume of EDTA stock to prepare buffer A which contains 10 mM EDTA with final volume is 100 ml by using M1V1 =M2V2 formula 5)Do the same for Buffer B calculations