Here DNA is made up of nucleotides(one base+phosphate+sugar)and described as double helical model in which nitrogen bases are arranged in such a way that it provides hydrophobic effects by burying bases interior of double helix increases its stability , they held together by hydrogen bonding and charge -charge interactions provide stability to extreme conditions.
Nitrogen bases undergoes keto-enol tautomezism here keto form (C=O) is called as lactam enol from is known as lactim(-OH) .At pH VALUE 7 keto from(more stable) is in highest amount that stabilizes the molecule and at the same time phosphate groups in DNA molecules are in negative charge at this pH charge -charge repulsion places this groups opposite direction stabilizes the molecule and room temperature it exists as highly viscous as the temperature increases it viscosity decrease that ultimately effects its physical and chemical properties
Why is DNA stable in an aqueous solution, at pH 7.0, and room temperature?
will have a pH of 7.0 at 25.0 °C. A 0.2 M aqueous solution of NaF NaCl NaClO4 RbBr O A. RbBr and NaClO4 O B. LiF and RbBr OC. NaClO4 only OD. LiF only O E NaCl, NaClO4, and RbBr
please show work Phenethicillin degrades at pH 7.0 in aqueous solution at 25°C by first-order kinetics with a half-life of 515 h. How many hours will it take for a solution of phenethicillin to degrade to 90% of its starting concentration? 01 d b 1931 aug od o borbenog gub to blow on ISO 2110 on loom S omnis ist to a
3. Consider a room temperature, 100mL aqueous solution saturated with the ionic compound beryllium hydroxide Be(OH)2 due to the addition of 10g of Be(OH)2; MM-43.02 g-mol-1. KsP-2.0 x10-8 Use this provided information to calculate the pH of this saturated solution. Hints: Due to the low solubility product, very little of this compound actually dissolves in H20. Go ahead and assume all activity coefficients are equal to 1.0 for this problem. This seems like a good opportunity to apply the ICE...
The [H+] concentration in an aqueous solution at room temperature is 1.4 x 10-6M. What is the [OH-] concentration? Group of answer choices S5.6 x 10-8 M 7.1 x 10-9 M 5.2 x 10-11 M 5.6 x 10-6 M
An aqueous solution is saturated in both lithium sulfate and nitrogen gas at room temperature? what is most likely to happen if temperature increase also what would happen if temperature decrease? a. More solid lithium sulfate is observed only b. More nitrogen bubbles are observed only c. More solid lithium sulfate and less nitrogen bubbles are observed d. Less solid lithium sulfate and more nitrogen bubbles are observed e. Nothing happens
Data and Tables Mass Temperature pH NaCl 5.Og 25.00 C 7.0 AgNO3 5.Og 25.00 C 7.0 lann pH Initial (before addition of water) After Addition of Water Final (when reaction concluded) Temperature 25. 0 0 45.02 25.0 6.8 7.0 Species Na Molarity 1.00481e-7 1.00481e-7 7.09719 4.65556 2.44163 3.93421e-11 NO3 AB Solid Product:ARCI Grams: 4.21853 Data analysis and calculations ayout Views Note that all of the aqueous species in the above reaction exists as ions in solution: NaClw exists as Nat...
please write clearly and circle answer thx 28) a) What is the pH of a 0.159 M aqueous solution of ammonium iodide, NHAI pH- This Solution is acid, basic, or neutral b) What is the pH of a 0.250 M aqueous solution of sodium acetate, NaCH3COO? pH- This Solution is acid, basic, or neutral c) The substance benzoic acid (C6HsCOOH) is a weak acid (Ka - 6.3x10-s) What is the pH of a 0.123 M aqueous solution of sodium benzoate,...
Part A At a certain temperature, the pH of a neutral solution is 7.41. What is the value of Kw at that temperature? Part B What is the H+ concentration for an aqueous solution with pOH = 4.15 at 25 ∘C?
Which of these statements are true for a neutral, aqueous solution at 25 °C? pH=7.00 pOH=7.00 [H+]=[OH−] Which of these statements are true for a neutral, aqueous solution regardless of temperature? pOH=7.00 [H+]=[OH−] pH=7.00
1) An acetic acid aqueous solution has a pKa of 4.76 and pH of 3.00. What is the concentration of acetic acid? 2) An experiment requires you to culture mammalian cells in 10 mL of culture medium buffered to a pH of 7.4 with 25 mM HEPES. After the experiment, the pH dropped to 7.0. How many equivalents of acid must have been produced by the cells to have dropped the pH?