Calculate the AH° of the borate dissolution at 25°C in kJ mol-1, if the 22.12 mL of 0.025 M HCIsolution used up to titrate 11.14 mL of saturated borax solution. AS of borax dissolution is 61.14J mol 1 K1, and gas constant is 8.314 J mol 1K1. Record the answer to two decimal places.Borax dissolution reaction:NagB.O7 • 10H20) 2 Na (ag) + B,O5(OH),le) + 8 H20)(aq)Reaction of borate anion with HCl:B,Os(OH),) + 3 H20) + 2 H (aq) → 4 B(OH)3(ag)(aq)

Solution- Given data- T= 250C =298K ∆S0 = 61.14 J mol-1 K-1, gas constant = 8.314 J mol-1 K-1

Calculate the AH° of the borate dissolution at 25°C in kJ mol1, if the 22.12 mL of 0.025 M HCI solution used up to titrate 11.14 mL of saturated borax solution. AS° of borax dissolution is 61.1 J mol 1 K1, and gas constant is 8.314 J mol1K1. Record the answer to two decimal places. Borax dissolution reaction: NagB,O7 • 10H2O 2 2 Na (ag) + B,05(OH),) + 8 H2O() (aq) Reaction of borate anion with HCl: B,O;(OH),) )4 B(OH)3(aq) +3 H2O+2 H (aq)

Calculate the AH° of the borate dissolution at 25°C in kJ mol1, if the 22.12 mL of 0.025 M HCI solution used up to titrate 11.14 mL of saturated borax solution. AS° of borax dissolution is 61.1 J mol 1 K1, and gas constant is 8.314 J mol1K1. Record the answer to two decimal places. Borax dissolution reaction: NagB,O7 • 10H2O 2 2 Na (ag) + B,05(OH),) + 8 H2O() (aq) Reaction of borate anion with HCl: B,O;(OH),) )4 B(OH)3(aq) +3 H2O+2 H (aq)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Q.1 -8 K, for HCO3 = 2.38 × 10 Calculate Ka for the conjugate acid ( H¿CO;) For the reaction : H2CO3(aq) + H2O(aq) HCO3 (aq) + H3O'(aq) Q.2 The molar solubility for Mg3(PO.); is 3.5 × 106M. Calculate the K, of Mg;(PO4)2 for the reaction: Mg:(PO4)2 (s) = 3 Mg* (aq) + 2PO,* (aq) The K, expression is: Ksp = [Mg²+ ]³ [PO4³ j²
5.
Calculate the solubility at 25 °C of AgCl in pure water and in 0.34 M NaCN. You'll probably find some useful data in the ALEKS Data resource. Round your answer to 2 significant digits. Solubility in pure water: Solubility in 0.34 M NaCN: 1.3 × 10 Ом -5 M x10
Calculate the pH at 25 °C of a 0.44M solution of potassium butanoate (KC,H,CO,). Note that butanoic acid (HC,H,CO,) is a weak acid with a p K, of 4.82. Round your answer to 1 decimal place. pH = 0
Tue Apr 11 TA ... B HO + 1. Write the chemical reaction for the titration of the filtered KHT solution in pure water.
For nos. 4 - 7: Consider a saturated solution of barium iodate in 0.025 M BaCl2. For the salt: Ba(1O3)2(s) Ba2+ + 2103 Ksp = 1.57 x 10-9 at 25°C %3D
The value of the thermodynamic solubility product of silver bromide in pure water is Ksp = 5.0x10-13. Calculate the value of the concentration solubility product of silver bromide in a 0.10 M NaNO3 solution. Let's assume the temperature is the same.
At 15 ° C and in pure water, the solubility of AgCl (silver chloride) is 8.4×10−5 mol.L-¹. The one of silver bromide (AgBr) is 3.8×10-7 mol.L-¹. What are their solubilities in a solution saturated by both the salts? The answer : s(AgCl) = 8.4×10−5 mol.L=1; s(AgBr) = 1.7×10-9 mol.L
Calculate the standard Gibbs energy change for the following reaction at 298 K H2(g) + Cl2(g) ® 2HCl(g) [DfHo = –92.3 kJ mol–1 for HCl; S in J K–1 mol–1 is 131, 223, and 187 for H2, Cl2 and HCl, respectively].
Consider the following mixtures of chemicals. Complete the table by writing balanced equations and calculating the value of Q. Hence indicate whethe precipitation will occur. Mixture Balanced equation Ksp Q Precipitation occurs (yes or no) 100mL 0.5 molL-1 Ca(NO3)2 mixed with 100 mL 0.2 molL-1 Na2SO4 20 mL 0.01 molL-1 AgNO3 mixed with 80 mL 0.05 molL-1 K2CrO4
sp Calculate the solubility at 25 °C of BaCrO4 in pure water and in a 0.0130M BaCl₂ solution. You'll find K data in the ALEKS Data tab. Round both of your answers to 2 significant digits. solubility in pure water: solubility in 0.0130 M BaCl₂ solution: 0 g g 0 -/-/ 00 x10 X Ś 00 G
TUOv to lls worla taum uo 1o9TIOoni bolam od lliw elimu iboo lut o 19 4. Given the Borax reaction below, what would be the solubility product (Ksp) of borax at 40 °C, if the solubility of borax is 0.8 mol L¯1 at 40 °C? Na,B4O5 (OH)4 · 8H,O(s) = 2Na+ (aq) + B405(OH) (aq) +8H,O(1) sr vol (A) gnsb vgotino brrbae ar bo CHO)gab xglerino bisbasie orb il S