Enroll in one of our FREE online STEM summer camps. Space is limited so join now!View Summer Courses

Ohio State University

Problem 1
Problem 2
Problem 3
Problem 4
Problem 5
Problem 6
Problem 7
Problem 8
Problem 9
Problem 10
Problem 11
Problem 12
Problem 13
Problem 14
Problem 15
Problem 16
Problem 17
Problem 18
Problem 19
Problem 20
Problem 21
Problem 22
Problem 23
Problem 24
Problem 25
Problem 26
Problem 27
Problem 28
Problem 29
Problem 30
Problem 31
Problem 32
Problem 33
Problem 34
Problem 35
Problem 36
Problem 37
Problem 38
Problem 39
Problem 40
Problem 41
Problem 42
Problem 43
Problem 44
Problem 45
Problem 46
Problem 47
Problem 48
Problem 49
Problem 50
Problem 51
Problem 52
Problem 53
Problem 54
Problem 55
Problem 56
Problem 57
Problem 58
Problem 59
Problem 60
Problem 61
Problem 62
Problem 63
Problem 64
Problem 65
Problem 66
Problem 67
Problem 68
Problem 69
Problem 70
Problem 71
Problem 72
Problem 73
Problem 74
Problem 75
Problem 76
Problem 77
Problem 78
Problem 79
Problem 80
Problem 81
Problem 82
Problem 83
Problem 84
Problem 85
Problem 86
Problem 87
Problem 88
Problem 89
Problem 90
Problem 91
Problem 92
Problem 93
Problem 94
Problem 95
Problem 96
Problem 97
Problem 98
Problem 99
Problem 100
Problem 101
Problem 102
Problem 103
Problem 104
Problem 105
Problem 106
Problem 107
Problem 108
Problem 109
Problem 110
Problem 111

Need more help? Fill out this quick form to get professional live tutoring.

Get live tutoring
Problem 84

$\mathrm{ABaSO}_{4}$ slurry is ingested before the gastrointestinal tract is $\mathrm{x}$ -rayed because it is opaque to $\mathrm{x}$ -rays and defines the contours of the tract. $\mathrm{Ba}^{2+}$ ion is toxic, but the compound is nearly insoluble. if $\Delta G^{\circ}$ at $37^{\circ} \mathrm{C}$ (body temperature) is 59.1 $\mathrm{kJ} / \mathrm{mol}$ for the process

$$\mathrm{BaSO}_{4}(s) \rightleftharpoons \mathrm{Ba}^{2+}(a q)+\mathrm{SO}_{4}^{2-}(a q)$$

what is $\left[\mathrm{Ba}^{2+}\right]$ in the intestinal tract? (Assume that the only source

of $\mathrm{SO}_{4}^{2-}$ is the ingested slurry.)

Answer

Check back soon!

You must be logged in to like a video.

You must be logged in to bookmark a video.

## Discussion

## Video Transcript

were given this soluble ity reaction and its value for the changing Gibbs free energy. It's danger conditions at a temperature of 37 degrees Celsius, which one converted into Kelvin, comes out to 310 from this information. At these conditions, we want to determine the concentration of be a two plus ions in solution and from the information in the problem, we can conclude that the concentration of be a two plus is equal to the concentration of S 04 to minus and solution so we can begin by reading out the equilibrium constant expression where K equals when we look at the acquia species. Participating in this reaction equals B A two plus that concentration value won't applied by concentration of s 04 tu minus. Based on this relationship, we can see that this equals the concentration of be a two plus squared. And we also know an equation to relate the equilibrium constant with the change in Gibbs free energy value. So once we solve for that value for K, we can take the square root of it to isolate and find the concentration of barium ions in solution. So the equation, their release K in Delta G is K equals E to the power of negative Delta G over rt So K equals e to the power of negative Delta G, which were given as 59.1 village als per mole. But we should convert that into jewels promotion that we can cancel out the units of the constant are so we should multiply that by 1000. Get it from killing jewels to Jules per mole. And then we divide that by the constant are 8.314 joules per mole times Kelvin times that temperature of 310 Kelvin. And now when we cancel off the units of Kelvin and jewels Permal, we can successfully take e to the power of this quantity. Since it is dimension lis and we come up with a you mentioned this value for or K two B equal to concentration of B A two plus squared so that when we take the square root of this K that we found from this equation, we can get a concentration of barium ions. You be equal to 1.5 times 10 to the power of negative five bulls for leader

## Recommended Questions