4. Draw a particulate (molecular level) representation of the solution mixture in the question above (Question 3). Do not include water molecules in your drawing.
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Question #4 please
![3. If the solution with the pH of 2.30 had a concentration of 0.05 M, what is the percent
ionized for the acidic solution?
pH=D2.30
C= 0.05 M
2.30
10 = 5. 01 X 10
0.100
%3D
0.05
[ amt dissoc)
X100
[Inifial con ]
5.01 X 10-4
0.05
10%0
X 1000
ニ
4. Draw a particulate (molecular level) representation of the solution mixture in the
question above (Question 3). Do not include water molecules in your drawing.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdc024bdf-b8f8-4bd4-bb69-1e67cee7f79e%2Fb1772c14-f92a-4351-8692-19020b9a460a%2F048qj8x_processed.jpeg&w=3840&q=75)
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- What is the pH of the solution after mixing 0.171 g of Mg(OH)2 (MW=58.321 g/mol) with 68.9 mL of 0.0569 M HCl? The resulting solution was diluted to 100 mL. Round your calculated value for pH to two figures to the right of the decimal point.What volume (mL) of 0.105 M HClO4 solution is required to neutralize 50.00 mL of 0.0805 M Ca(OH)2 ?The pH and electrical conductivity of four different mixtures were measured: Mixtures conductivity (mA) pH a. 0.1 mol L-1 HCI 260 1 B. 0.1 mol L-1 CH3COOH 5 3 c. Mixture made by mixing equal volumes of 0.2 mol L-1 HCI and 0.2 mol L-1 NaCl 340 1 D. Mixture made by mixing equal volumes of 0.2 mol L-1 HCI and 0.2 mol L-1 NaCH3COO 80 3 a. Explain why the conductivity of mixture a is higher than that of mixure b, yet the pH of a is lower than the pH of B. Include relevant equations in your answer b. Explain why the pH of mixture C is the same as the pH of mixture A c. Why is the conductivity of mixture C larger than the conductivity of mixture A d. Why is the pH of mixture D the same as the pH of mixture B Determine the final pH for the following two solutions a. solution a after mixing 500 ml 0.2M HCl and 300 ml 0.6M Hcl b. solution b after mixing 400ml 0.3M HCl and 200ml 0.8M NaOH
- Give typed explanation of all subparts The Concentration of Mg2+ ions in seawater is 5.37 x 10-2 M. Calculate the pH at which Mg2+ is decreased to 1.0 x 10-5 M. Ksp of Mg(OH) is 8.9 x 10-12. Writing the balance equation Writing the expression for the Ksp Plugging the terms for Ksp Calculating OH- concentration Calculation of pHThe pH and electrical conductivity of four different mixtures were measured:Mixtures Conductivity(mA)pHA 0.1 mol L–1 HCl 260 1B 0.1 mol L–1 CH3COOH 5 3C Mixture made by mixing equal volumes of0.2 mol L–1 HCl and 0.2 mol L–1 NaCl340 1D Mixture made by mixing equal volumes of0.2 mol L–1 HCl and 0.2 mol L–1 NaCH3COO80 3 Explain why the conductivity of mixture A is higher than that of mixture B, yet the pH of A is lower than the pH of B. Include relevant equations in your answer. Explain why the pH mixture of C is the same as the pH mixture of A. Why is the conductivity of mixture C larger than the conductivity of mixture A? Why is the pH of mixture D the same as the pH of mixture B?The pH and electrical conductivity of four different mixtures were measured: Mixtures Conductivity (Ma) PH a) 0.1 mol L-1 HCl 260 1 b) 0.1 mol L-1 CH3OOH 5 3 c) Mixture made by mixing equal valumes of 0.2 mol L-1 HCl and 0.2 mol L-1 NaCl 340 1 d) Mixture made by mixing equal volumes of 0.2 mol L-1 HCl and 0.2 mol L-1 NaCH3COO 80 3 a) Explain why the conductivity of mixture A is higher than that of mixture B, yet the pH of A islower than the pH of B. Include relevant equations in your answer. b) Explain why the pH of mixture C is the same as the pH of mixture A. c) Why is the conductivity of mixture C larger than the conductivity of mixture A? d) Why is the pH of mixture D the same as the pH of mixture B? Part B – Determine the final pH for the following two solutions a) Solution A after mixing 500mL 0.2M HCl and 300 mL 0.6M HClb) Solution B after mixing 400mL 0.3M HCl and 200mL 0.8M NaOH
- the pH and electrical conductivity of four different mixtures were measured mixtures conductivity (mA) pH a. 0.1 mol L-1 HCl 260 1 b. 0.1 mol L-1 CH3COOH 5 3 c. mixture made by mixing equal volumes of 0.2 mol L-1 HCl and 0.2 mol L-1 NaCl 340 1 d. mixture made by mixing equal volumes of 0.2 mol L-1 HCl and 0.2 mol L-1 NaCH3COO 80 3 Determine the final pH for the following two solutions a) solution A after mixing 500ml 0.2M HCl and 300ml 0.6M HCl b) solution B after mixing 400 ml 0.3M HCl and 200 ml 0.8M HClthe pH and electrical conductivity of four different mixtures were measured mixtures conductivity (mA) pH a. 0.1 mol L-1 HCl 260 1 b. 0.1 mol L-1 CH3COOH 5 3 c. mixture made by mixing equal volumes of 0.2 mol L-1 HCl and 0.2 mol L-1 NaCl 340 1 d. mixture made by mixing equal volumes of 0.2 mol L-1 HCl and 0.2 mol L-1 NaCH3COO 80 3 C. Why is the conductivity of mixture C larger than the conductivity of mixture a? D. Why is the pH of mixture D the same as the pH for mixture B?What volume of 0.060 M H2SO4 will neutralie 50.00mL of 0.24M NaOH? The answer is 100mL
- Five solutions A, B, C, D and E when tested with universal indicators showed pH as 4, 1, 11, 7 and 9 respectively. Which solution is:(a) neutral?(b) strongly alkaline?(c) strongly acidic(d) weakly acidic?(e) weakly alkalineCalculate the pH of a solution of 0.01 M NaF, given Kb for F- = 1.4 x 01-11. Group of answer choices 8.08 7.57 6.43 2.0What volume of 0.300 M H2SO4 can be made from 15.5 mL of 0.624 M H2SO4? 2. Calculate the volume of 2.57 M NaOH needed to make a 470. mL solution of 0.0500 M NaOH.